Web viewUse the numbers given to me in word problems to solve the wavelength ... change during thermodynamic ... molarity of a solution given grams

Name ___________________

Chemistry Review

Chm.1.1 Matter:Properties and Change Chm. 1.1.1 Analyze the structure of atoms, isotopes, and ions.

Chm. 1.1.2 Analyze an atom in terms of the location of electrons.

Chm. 1.1.3 Explain the emission of electromagnetic radiation in spectral form in terms of the Bohr model

Chm. 1.1.4 Explain the process of radioactive decay by the use of nuclear equations and half-life.

Big Ideas Essential Questions

Know the location and charge of protons, neutrons, electrons

Determine an element’s number of protons, electrons, and neutrons based off the given isotopic symbols

Differentiate average atomic mass of an element from the actual isotopic mass and mass number of specific isotopes

Analyze electrons in terms of

• Bohr model

• Excited stated vs. ground state

• Emission spectrum (Reference Table)

• electron configurations

• wave/particle duality

Understand the inverse relationship between wavelength and frequency, and the direct relationship between energy and frequency.

Write and balance nuclear equations

Describe nuclear decay

Compare fission and fusion

Understand half-life problems

How can atomic models be used to describe and explain the structure of atoms?

In what ways has the theory of the atom changed over time due to technological developments?

What is the law of conservation of mass?

What is the law of definite proportions/multiple proportions?

What were the 5 points to Dalton’s atomic theory?

How was the use of cathode rays responsible for the discovery of the electron?

How did Rutherford’s experiment lead to the discovery of the atomic nucleus?

What are the properties (charge, mass, position) of protons, neutrons, and electrons?

What is an isotope? What is the atomic number of an

atom equal to? What is the mass number of an

atom equal to? Why is the mass number in the

periodic table a decimal? How is the wave-particle duality

explanation used to explain light and electrons?

What is the relationship between the speed, frequency, and wavelength of electromagnetic

radiation? What is the significance of the

photoelectric effect in describing the behavior of the electron and light?

How did the Heisenberg Uncertainty Principle and the Schrödinger Wave equation lead to atomic orbitals?

What are the downfalls of the Bohr model of the atom?

What are the differences between the Bohr model and the Quantum model of the atom?

What is the significance of each of the four quantum numbers?

How are the quantum numbers used to describe the position of an electron in an atom?

How many electrons fill each energy level and each orbital?

What is the significance of the Aufbau principle, the Pauli Exclusion Principle, and Hund’s rule when discussing electron configuration within the atom?

Given an element, how do I determine its electron configuration, orbital notation, and electron dot notation?

How are nuclear reactions used to describe nuclear decay

How do nuclear fission and nuclear fusion reactions differ?

Atom

Atomic mass

Atomic mass unit

Atomic number

Electron

Ion

Isotope

Mass number

Neutron

Nucleus

Emission Spectra

Energy level

Orbital

SublevelElectromagnetic radiation

Emission spectra

Energy

Energy level

Frequency

Nucleus

ProtonBohr Model

Electron

Electron cloud

Electron configurations

Orbital

Photon

Quanta

Sublevel

WavelengthFission

Fusion

Half life

Nuclear Decay

Radioactive decay

Student Performance Goals

Learning Targets Criteria for Success

I will… I can…

Be able to look at the periodic table and determine the number of protons, electrons and neutrons and elements has

Determine number of protons, electrons, and neutrons when given an isotopic symbol

Tell the difference between average atomic mass and mass number

Draw an elements Bohr Model Be able to determine electron

configurations for elements Manipulate and solve C = Use and understand the

electromagnetic spectrum Be able to write and balance nuclear

equations use alpha and beta particles

Explain nuclear fission and fusion Successfully work through half-life

problems

Correctly calculate the number of protons, neutrons and electrons for all elements

Describe the difference between average atomic mass and mass number

Correctly draw Bohr Models for all elements making sure to include the nucleus and energy levels in which to place the electrons

Write the correct electron configurations for all elements making sure to include the s, p, d, f in the appropriate order

Use the numbers given to me in word problems to solve the wavelength formula and then use the numbers locate the appropriate area on the electromagnetic spectrum

Correctly write and balance nuclear equations using the knowledge that undergoing alpha decay produces an alpha particle and undergoing beta decay produces a beta particle.

Correctly describe nuclear fission is the splitting of one nucleus into two or more smaller nuclei and nuclear fusion is the joining of two or more

nuclei into one nucleus Use given information to solve

radioactive half-life problems

Chm. 1.2 Understand the bonding that occurs in simple compounds in terms of bond type, strength, and properties

Chm. 1.2.1 Compare (qualitatively) the relative strengths of ionic, covalent, and metallic bonds

Chm. 1.2.2 Infer the type of bond and chemical formula formed between atoms

Chm. 1.2.3 Compare inter- and intra- particle forces

Chm. 1.2.4 Interpret the name and formula of compounds using IUPAC convention

Chm. 1.2.5 Compare the properties of ionic, covalent, metallic, and network compounds


Predict bond type based off location of elements on the periodic table

Determine positive and negative charge of element based off location of element on periodic table

Predict chemical formulas

Write and name binary chemical formulas/compounds

Write and name compounds using Polyatomic Ions

Know names and formulas for common acids

Describe intermolecular forces for molecular compounds

Explain the strengths and characteristics of intermolecular forces, ionic, covalent, and metallic bonds

Explain the strengths of hydrogen bonds, dipole-dipole forces, and London Dispersion forces

Apply and explain VSEPR with respect to molecular geometry

Compare/Contrast polarity vs. nonpolarity

Describe macromolecules and network solids

How does the distribution of electrons in atoms affect the formation of a compound?

What factors determine the types of chemical bonds that form between particles?

How do elements form ionic bonds? How do elements form covalent

bonds? Are all electrons shared equally? How are the properties of metals

explained through metallic bonding?

How are the names of compounds determined (inorganic and acids)?

How are the formulas for compounds written?

How can I translate between a compound's name and its formula?

How can the charges of ions be used to determine balanced formulas involving polyatomic ions?

How can we predict the shape, structure and properties of molecules?

What is the difference between ionic, covalent, and metallic bonding?

How do intramolecular and intermolecular forces affect

properties of a compound?

Anion

Cation

Covalent Bond

Electron Dot Structure/Diagram (Lewis Dot Structure/Diagram)

Ionic Bond

Metallic Bond

Valence Electron

Chemical Formula

Ionic Bond

Lewis Structure

Periodic TableCovalent Bond

Diatomic Molecule

Dipole-Dipole Forces

Hydrogen Bond

Intermolecular Forces

Intramolecular Forces

Ionic Bond

London Dispersion Forces

Metallic Bond

Polar Bond

Binary Compound

Metal

Molecule

Nomenclature

Nonmetal

Polyatomic Ion

Covalent Bond

Ionic Bond

Ionic Compound

London Dispersion Forces

Metallic Bond

Molecular Compound

van der Waals Forces

VSEPR


I will… I can…

Be able to distinguish the difference between bond type and characteristics

Be able to predict bond type when given elements

Be able to draw ionic bonding diagrams

Write chemical formulas Name chemical compounds Write chemical formulas and name

compounds using polyatomic ions Determine VSEPR Shape Determine Polarity/NonPolarity Be able to explain intermolecular

forces Be able to distinguish between a

network solid and a macromolecule.

Explain the characteristics of covalent, ionic, and metallic bonds

Examine elements given and based off their location on the periodic table determine if they will form a binary covalent, ionic, or metallic bond

Use Lewis structures to draw ionic bonding diagrams

Use ionic bonding diagrams to determine cationic and anionic charges of the elements.

Determine charges of elements and use the cross down method to write chemical formulas

Use the correct IUPAC systems (include Stock and Greek Systems) to correctly name compounds

Name and write compounds containing polyatomic ions

Draw the correct molecular geometry shape for covalent

compounds and determine the correct VSEPR shape

Explain the concept behind the VSEPR theory

Draw correct VSEPR shapes for covalent compounds and determine if they are polar or nonpolar

Explain the difference between inter- and intramolecular forces

Explain the differences between all the intermolecular forces

Distinguish the difference between a macromolecule and a network solid

Chm. 1.3 Understand the physical and chemical properties of atoms based on their position on the Periodic Table

Chm. 1.3.1 Classify the components of a periodic table (period, group, metal, metalloid, nonmetal, transition)

Chm. 1.3.2 Infer the physical properties (atomic radius, metallic and nonmetallic characteristics) of an elements based on its position on the Periodic Table

Chm. 1.3.3 Infer the atomic size, reactivity, electronegativity, and ionization energy of an element from its position on the Periodic Table.


Identify groups as vertical columns on the periodic table

Know that main group elements have similar properties, have the same number of valence electrons, and same oxidation numbers

Identify periods as horizontal rows on the periodic table

Know the location of metals, nonmetals, and metalloids on the periodic table

Use electron configuration to justify metallic character

Using the periodic table, define and know the period and group trends of:

• Atomic radius

• Electron affinity

• Ionization energy

• Electronegativity

How does the placement of an element in the Periodic Table relate to its chemical and physical properties?

How does knowing trends on the Periodic Table help scientists predict properties of the representative elements?

What happens to the atomic radius as the atomic number increases across a period? Down a group?

What happens to the energy needed to remove an electron as the atomic number increases across a period? Down a group?

Why does atomic radius change as it does?

Why does the energy required to remove an electron change as it does?

Arrange elements in order of increasing or decreasing atomic radius/electron affinity/ionization energy/electronegativity and explain reasoning behind the trend.

Alkali Metal

Alkali Earth Metal

Group (Family)

Halogen

Meta

Metalloid

Noble Gas

Nonmetal

Oxidation Number

Period, Reactivity

Transition Element

Valence Electron

Anion Radius

Atomic Radius

Cation Radius

Electron Affinity

Electron Configuration

Electronegativity

Ionic Radius

Ionization Energy

Metallic Character

Octet

Oxidation Number

Valence Electron

Electronegativity

Ionization Energy

Reactivity


I will… I can…

Describe the arrangement of the modern Periodic Table in terms of identifying families

Describe elements in terms of number of metallic character, number of valence electrons, and number of oxidation numbers

State the general trend for and arrange elements according to

o Atomic and ionic radiuso Ionization energyo Electronegativityo Metallic charactero Electron affinity

Be able to determine if elements will gain or lose electrons based off position on Periodic Table

Be able to arrange a group of 3 or 4 elements in increasing or decreasing order according to desired trend (atomic radius, ionization energy, ionic radius, electronegativity, electron affinity)

Be able to tell if elements are in the same family and have the same number of energy levels based off given properties

Chm.2.1 Energy: Conservation and TransferChm. 2.1 Understand the relationship among pressure, temperature, volume, and phase

Chm. 2.1.1 Explain the energetic nature of phase changes

Chm. 2.1.2 Explain heating and cooling curves (heat of fusion, heat of vaporization, melting point, and boiling point)

Chm. 2.1.3 Interpret the data presented in phase diagrams

Chm. 2.1.4 Infer simple calorimetric calculations based on the concepts of heat lost equals heat gained and specific heat

Chm. 2.1.5 Explain the relationships among pressure, temperature, volume, and quantity of gas, both qualitative and quantitative


All chemical and physical changes involve energy transfer

The amount of heat transferred in a chemical/physical change can be predicted (calculated) using a balanced chemical equation. It can also be measured quantitatively through experimental means and graphically represented

Explain why gases are less soluble in warm water than cold water

Investigate the difference in the boiling or freezing point of pure water and a salt solution

Measure, plot, and interpret the graph of a phase diagram of a substance under various conditions

Examine and interpret heating and cooling curves for various closed systems.

Contrast heat and temperature, including temperature as a measure of average kinetic energy

Know that energy is neither created nor destroyed

Explain physical equilibrium Explain and understand the relationship

between pressure, temperature, volume, and amount of gas

Complete calculations of:

How is energy transferred in chemical systems?

How does the potential energy and kinetic energy of molecules change during thermodynamic processes?

How do heat, temperature and internal energy differ?

Why is absolute zero so named? Why can all reactions be classfiied

as exothermic and endothermic? How much energy is required to

change a substance? How is energy converted between

kinetic energy and potential energy in a chemical reaction?

How does the motion of particles affect the temperature and phase of a substance?

How does pressure affect particle motion and phase change?

What is the relationship between molecular motion and thermal energy?

What is the nature of energy transfer?

How do you calculate heat capacity?

How do gases behave?

How do changes in pressure, volume, and temperature affect a gas?

What impact does the world of gases have on your life?

What are the key parameters that define a gas?

How are pressure and volume

related to each other? How are volume and temperature

related to each other? How are temperature and pressure

related to each other? How does Kinetic Molecular Theory

describe the behavior of gases? What is pressure? How does a gas exert pressure? How do we measure pressure?

Celsius

Equilibrium

Joule

Kelvin

Kinetic Energy

Phase

Phase Change

Physical Equilibrium

Potential Energy

Vapor Pressure

Boiling Point

Cooling Curve

Endothermic

Exothermic

Heat of Fusion

Heat of Vaporization

Heating Curve

Melting Point

Specific Heat

Boiling Point

Melting Point

Phase Diagrams

Sublimation

Calorimetry

Closed System

Phase Change

Specific Heat

Avogradro’s Law

Combined Gas Law

Dalton’s Law

Ideal Gas Law

Kinetic Molecular Theory

Pressure

Solubility

Temperature

Volume


I will… I can…

Be able to interpret and construct phase diagrams

Be able to interpret and construct heating/cooling curves

Explain the difference between heat and temperature

Explain the relationship between temperature and kinetic energy

Explain how vapor pressure is dependent upon temperature and concentration

Solve word problems using the energy and gas law formulas

Explain the differences between an ideal and real gas

Correctly construct a phase diagram for water and carbon dioxide

Correctly interpret and read phase diagrams for any substance

Correctly interpret and design energy diagrams for any substance

Describe the differences between endothermic and exothermic reactions

Use the following formulas to solve given word problems and explain the outcome:

Explain gas solubility rules and characteristics

Explain temperature is the average molecular movement of particles and more molecular movement will equal more kinetic energy

2.2 Analyze chemical reactions in terms of quantities, product formation, and energy

Chm.2.2.1 Explain the energy content of a chemical reaction.

Chm.2.2.2 Analyze the evidence of chemical change.

Chm.2.2.3 Analyze the law of conservation of matter and how it applies to various types of chemical equations (synthesis, decomposition, single replacement, double replacement, and combustion).

Chm.2.2.4 Analyze the stoichiometric relationships inherent in a chemical reaction.

Chm.2.2.5 Analyze quantitatively the composition of a substance (empirical formula, molecular formula, percent composition, and hydrates).


Relate collision theory to activation energy.

Interpret potential energy diagrams

Know the evidences of chemical change.

How do I explain collision theory? How must molecules collide in order to react? What must be achieved before a reaction occurs in terms of energy? How are potential energy diagrams interpreted? What are the differences between the diagrams of exothermic and endothermic

reactions? Where on a potential energy diagram is the activated complex located? What is the

significance of the activated complex? What are the criteria used to determine whether or not a chemical reaction has

occurred? What is a precipitate and how can solubility rules be used to predict precipitate

formation? How can I test for the presence of hydrogen being produced in a reaction?

Recognize reactions by type.

Predict products of synthesis, decomposition, single replacement, double replacement, and combustion reactions.

Balance reactions using the law of conservation of matter and coefficients.

Perform stoichiometric calculations in different units (grams, moles, liters, molecules, etc.)

Calculate empirical and molecular formulas.

Calculate percentage composition of compounds and hydrates.

How can I test for the presence of oxygen in a chemical reaction? How can yI test for the presence of carbon dioxide being produced in a chemical

reaction? How can I test for the presence of water produced in a chemical reaction? How does absorption and release of heat indicate that a chemical change occurs? What are the signs of ∆H for endothermic and exothermic reactions? How do I predict products and balance chemical reactions once the type of reaction is

known? How do I identify the type of reaction, given the reactants? How do I identify a double replacement reaction as acid-base neutralization? How do I write and balance ionic reactions? How do I write and balance net ionic reactions? What does a net ionic reaction show? How do I recognize combustion reactions? What are hydrocarbons? How can hydrocarbons be identified by the elements in their

formulas? How can I predict products to show how the law of conservation of mass is satisfied? How do I use the activity series to predict products of single replacement reactions? How do I use solubility rules to predict whether or not a precipitate will occur in a

double replacement reaction when both reactants are aqueous? What do coefficients in balanced reactions represent? How do I perform stoichiometry calculations given grams, moles, liters and particles

and finding grams, moles, liters and particles? How do I convert between units using the definitions of:1 mol= 6.02 X 1023 atoms, molecules particles, formula units1 mol = grams of an element or compound1 mol of a gas at STP= 22.4L

How do I calculate the empirical formula given percentage composition data for a compound?

How do I calculate the molecular formula of a compound given the empirical formula and the molar mass?

How do I calculate the molecular formula given the molar mass and percentage composition data for the compound?

How do I determine the percentage composition by mass of a compound? How do I perform calculations based on percent composition? How do I interpret lab data to find the composition of a hydrate?

endothermic

exothermic

potential energy

reactants

products

double replacement

mole ratio

molecular weight

stoichiometry

empirical formula

molecular formula

molecular weight

products

reactants

activated complex

activation energyreactants

products

precipitate

hydrocarbon

combustion

ionic equations

net ionic equations

single replacement

activity series

solubility rules

synthesis

reactants

products

law of conservation of matter

percentage composition

hydrates

law of conservation of matter



I will… I can…

Be able to explain collision theory. Interpret potential energy diagrams for

endothermic and exothermic reactions including reactants, products, and activated complex.

Be able to determine if a chemical reaction has occurred based evidence of chemical changes and reaction thermodynamics.

Be able to write and balance chemical equations predicting product(s) in a reaction using the reference tables.

Be able to identify acid-base neutralization as double replacement.

Be able to write and balance ionic and net ionic equations.

Be able to identify combustion reactions. Be able to use reference table rules to predict

products for all types of reactions to show the conservation of mass.

Be able to use activity series to predict whether a single replacement reaction will take place.

Be able to use the solubility rules to determine the precipitate in a double replacement reaction if a reaction occurs.

Be able to interpret coefficients of a balanced equation as mole ratios.

Be able to use mole ratios from the balanced equation to calculate the quantity of one substance in a reaction given the quantity of another substance in the reaction.

Be able to calculate empirical formula from mass or percent using experimental data.

Be able to calculate molecular formula from empirical formula using molecular weight.

Discuss the need for effective collisions between molecules in order to overcome activation energy and react.

Interpret potential energy diagrams so that the activated complex, reactants, products, change in enthalpy can be determined.

Identify exothermic and endothermic reactions from potential energy diagrams.

Determine whether or not a chemical reaction has occurred by looking for precipitate formation, color change, production of gases(hydrogen, oxygen, carbon dioxide, and water vapor), or temperature change.

Distinguish between color change as a result of new substances being made and dilution with water.

Show that the enthalpy change is negative for an exothermic reaction using lab data and that the enthalpy change is positive for an endothermic reaction using lab data.

Use the reference tables to identify types of reactions given reactants.

Predict products of reactions once the type is identified.

Balance reactions using the lowest whole number coefficients to satisfy the law of conservation of matter.

Write and balance ionic reactions. Write and balance net ionic reactions. Write and balance acid base neutralization

reactions. Write and balance combustion reactions. Identify hydrocarbons as compounds containing

Be able to determine percentage composition by mass of a given compound.

Be able to perform calculations based on percent composition.

Be able to determine the composition of hydrates using experimental data.

C and H. Use the activity series of metals and of halogens

to predict products of single replacement reactions if they occur.

Use the solubility rules in conjunction with double replacement reactions to predict if an insoluble precipitate will form.

Interpret coefficients as mole ratios in a balanced reaction when performing stoichiometric calculations.

Work stoichiometry problems given grams, moles, molecules, particles, liters (for gases) and looking for grams, moles, molecules, particles, liters (for gases).

Determine the empirical formula for a compound given percentage composition data.

Determine the molecular formula for a compound given the empirical formula and molar mass.

Determine the molecular formula given the molar mass and percentage composition data.

Determine the percentage composition by mass of a compound.

Determine the formula for a hydrate by using experimental data such as the mass of the compound before and after heating.

Chm.3.1 Interaction of Energy and Matter

Chm.3.1 Understand the factors affecting rate of reaction and chemical equilibrium.

Chm.3.1.1 Explain the factors that affect the rate of a reaction (temperature, concentration, particle size and presence of a catalyst).

Chm.3.1.2 Explain the conditions of a system at equilibrium.

Chm.3.1.3 Infer the shift in equilibrium when a stress is applied to a chemical system (Le Chatelier’s Principle).


Know the factors that affect the rate of a reaction.

Explain how the number of effective

How are reaction rate and number of effective collisions related?

What are the factors that affect the

collisions affects the reaction rate by changing temperature, pressure, concentration and adding a catalyst.

Analyze the factors that affect the equilibrium in balanced reactions.

Know that the equilibrium constant expression measures the extent that a reaction proceeds to equilibrium.

Understand Le Chatelier’s principle and how it explains the effects of concentration, temperature, pressure on the equilibrium.

Know that the entropy change in a reaction is related to the equilibrium shift.

number of collisions in a reaction? How do increases in temperature,

pressure, concentration and surface area affect the number of collisions in a reaction?

How does a catalyst increase the rate of reaction?

What is chemical equilibrium? What type(s) of reactions reach

equilibrium? How are equal rates of reactions and

equal concentrations of reactants/products related?

How are equilibrium constant expressions for reactions written?

How are equilibrium constant expressions evaluated as a measure of the extent that a reaction proceeds to completion?

What does the value of the equilibrium constant expression express?

What are some factors that affect the equilibrium?

How do temperature, pressure, and concentration affect the equilibrium of a reaction?

How is the shift in equilibrium in response to a stress related to the entropy change of the reaction?

pressure

concentration

surface area

catalyst

collision

energetics

kinetic energy

order

reactant

product reaction rate

Chemical equilibrium

Equilibrium expression

Equilibrium constant

Le Chatelier’s principle

Reactant

Product

Heat

Pressure

Order Disorder

Equilibrium

Le Chatelier’s Principle


Learning Targets Criteria for SuccessI will… I can…

Understand qualitatively

that reaction rate is proportional to number of effective collisions.

Be able to explain that nature of reactants can refer to their complexity and the number of bonds that must be broken and reformed in the course of reaction.

Be able to explain how temperature (kinetic energy), concentration, and/or pressure affect the number of collisions.

Be able to articulate how increased surface area increases number of collisions.

Be able to explain how a catalyst lowers the activation energy, so that at a given temperature, more molecules will have energy equal to or greater than the activation energy.

Define chemical equilibrium for reversible reactions.

Be able to distinguish between equal rates and equal concentrations.

Be able to explain equilibrium expressions for a given reaction.

Be able to evaluate equilibrium constants as a measure of the extent that the reaction proceeds to completion

Be able to determine the effects of stresses on systems at equilibrium.

Describe the effect of collisions among molecules on the reaction rate.

Look at the formulas for compounds in reactions and know that energy is stored in bonds that are formed and broken during a chemical reaction.

Determine how the reaction rate will be affected by changes in the temperature, pressure, and concentration of reactants or products.

Describe how the number of collisions among molecules is affected by using smaller or larger particles to perform the reaction.

Analyze lab data concerning the reaction rate and changing the temperature or concentration of a reactant.

Interpret reaction energy diagrams for catalyzed and uncatalyzed reactions.

Discuss the purpose of equilibrium constant expressions and show that when Keq=1 the reaction is at equilibrium, when Keq<1 the reaction is making reactants (shifting left), and when Keq>1 the reaction is making products(shifting right).

Determine the correct equilibrium constant expression for a reaction as

Use Le Chatelier’s Principle to determine which way a reaction at equilibrium will shift in response to a stress such as increasing/decreasing the temperature, adding/removing a reactant or product, adding a catalyst, and for gases increasing/decreasing the temperature.

Articulate in terms of entropy changes, why the equilibrium shifts in response to stresses added.

Explain the applications of Le Chatlier’s Principle in the lab and industry.

Analyze lab data obtained by adding or

(Adding/ removing a reactant or product; adding/removing heat; increasing/decreasing pressure)

Be able to relate the shift that occurs in terms of the order/disorder of the system.

removing reactants/products or increasing/decreasing the temperature using Le Chatelier’s Principle.

Chm.3.2 Interaction of Energy and MatterChm.3.2 Understand solutions and the solution process.

Chm.3.2.1 Classify substances using the hydronium and hydroxide ion concentrations.

Chm.3.2.2 Summarize the properties of acids and bases.

Chm.3.2.3 Infer the quantitative nature of a solution (molarity, dilution, and titration with a 1:1 molar ratio).

Chm.3.2.4 Summarize the properties of solutions.

Chm.3.2.5 Interpret solubility diagrams.

Chm.3.2.6 Explain the solution process.


Know the properties of acids and bases. Know how to calculate pH, pOH, [H+1], and [OH-

1] using formulas given in the reference tables. (pH=-log [H+1], pOH=-log [OH-1], [H+1]=10-pH, and [OH-1]=10-pOH )

Understand the pH an pOH scale Understand the purpose and use of indicators. Use lab data and solve problems with

concentration molarity and titration data. Understand the properties of solutions. Know the concept of solubility and be able to

interpret solubility graphs Understand the nature and energetics of the

solution process.

How do I identify acids and bases based on the chemical formula?

How do I identify acids and bases based on chemical and physical properties?

What is the relationship between concentration of solutions and the degree of dissociation?

How is the pH /pOH scale used to determine acidity /basicity of a solution?

How is the pH/pOH related to the concentration of hydrodgen/hydroxide ions in a solution?

How do I use indicators to determine the pH of a solution?

What are the different indicators used to determine the acidity of solutions?

How do I calculate pH, pOH, [H+1], and [OH-1] given the formulas provided in the reference tables? (pH=-log [H+1], pOH=-log [OH-1], [H+1]=10-pH, and [OH-1]=10-pOH )

What information do the values of pH, pOH, [H+1], and [OH-1] provide about a solution?

How do I calculate the molarity of a solution given grams and the volume of water? (using formula: M= moles of solution / liter of solution)

How do I calculate the grams of solute necessary to make a given volume of solution with a known molarity?(using formula M= moles of solute / liter of solution

How do I solve dilution problems given molarity and volume data?(using formula M1V1=M2V2)

How do I solve titration problems for an unknown molarity?(using formula M1V1=M2V2)

How are titration curves interpreted to determine the properties of the acid and base titrated?

How can titration curves be used to determine the end point and equivalence point of a titration?

What are the properties of solid, liquid, aqueous, and gaseous solutions?

Why are solutions considered homogenous mixtures?

What are the quantitative characteristics of the solutes and the solvent as compared to the whole solution?

What are the characteristics of electrolytic and nonelectrolytic solutions?

How is the electrical conductivity of a solution determined?

What are colligative properties? What causes colligative properties? What are the qualitiative consequences of

adding solutes to pure liquids in terms of the vapor pressure, the boiling point, the freezing point, and the osmotic pressure of the resulting solution?

What are the properities that solubility of a substance is dependent on?

How is the solubility of a substance related to the type of compound (ionic or covalent) as the temperature changes?

How is the solubility of a substance related to the state of matter (solid or gas)as the temperature changes?

How can I determine the solubility of a substance using a solubility graph?

How can I use a solubility graph to tell whether

a solution is saturated, unsaturated, or supersaturated at a given temperature?

How are the forces of attraction (intermolecular forces) related to the solubility of the solution?

How can I show using particle diagrams the forces of attraction among soluble and insoluble particles that make up solutions?

How is the heat transfer (released or absorbed) related to the dissolving process?

How can I determine whether dissolving is an endothermic or exothermic process?

How is solubility related to the attraction of the solute and solvent as the temperature is changed?

How is the solubility of a gas related to the attraction of the solute and solvent as the pressure is changed?

[H+1]

[OH-1]

Acid

Base

Concentration

Hydronium

Hydroxide

pH

pOH

Molarity

Dissociation

Titration

pH scale

Litmus paper

Phenolphthalein

Electrolytic solution Electrical conductivity

Nonelectrolytic solution

Acid

Base

pH

Molarity

Dilution

Concentration

Titration

Titration curve

Molar ratio

Electrolytic solutions Electrical conductivity

Nonelectrolytic solutions

Colligative properties Freezing point depression Boiling point elevation

Osmotic pressure

Vapor pressure reduction

Solubility Solubility diagrams Saturated

Unsaturated

Supersaturated

Solute-solvent attraction

Soluble

Insoluble


I will… I can…

Be able to distinguish between acids and bases based on formula and chemical properties.

Be able to differentiate between concentration (molarity) and strength (degree of dissociation). No calculation involved.

Be able to use the pH scale to identify acids and bases.

Be able to interpret pH scale in terms of the exponential nature of pH values in terms of concentrations.

Relate the color of indicator to pH using pH ranges provided in a table.

Be able to compute pH, pOH, [H+1], and

[OH-1].

Be able to distinguish properties of acids and bases related to taste, touch, reaction with metals, electrical conductivity, and identification with indicators such as litmus paper and phenolphthalein.

Be able to compute concentration (molarity) of solutions in moles per liter.

Be able to calculate molarity given mass of solute and volume of solution.

Be able to calculate mass of solute needed to create a solution of a given molarity and volume.

Be able to solve dilution problems: M1V1 = M2V2.

Perform 1:1 titration calculations: MAVA = MBVB

Be able to determine the concentration of an acid or base using a titration. Interpret titration curve for strong acid/strong base.

Be able to identify types of solutions (solid, liquid, gaseous, aqueous).

Define solutions as homogeneous mixtures in a single phase.

Distinguish between electrolytic and nonelectrolytic solutions.

Summarize colligative properties (vapor pressure reduction, boiling

Distinguish between acids and bases on the basis of the chemical formula and physical and chemical properties.

Differentiate between strong acids/bases and weak acids/bases by knowing the molarity and concentration.

Use the pH/pOH scales to identify acids and bases.

Understand the logarithmic nature of the pH/pOH scales

Use indicators to determine the acidity/basicity of solutions based on numbers and/or color changes and tables

Calculate pH, pOH, [H+1], and [OH-1] using the formulas given in the reference tables.

Perform experiments and analyze lab data to distinguish acids and bases using indicators and physical properties.

Work problems given grams and volume to find molarity of solutions.

Work problems given molarity and volume to find grams of solute required to make solutions.

Solve problems related to dilutions and titrations to find unknown volumes or molarities.

Perform titrations in the lab to determine an unknown molarity of a solution such as vinegar or how much of a substance is neutralized such as aspirin.

Interpret titration curves by finding the end point, equivalence point, the pH at the equivalence point and the strength of the acid and base titrated.

Identify solutions based on physical properties such as state of matter, electrical

point elevation, freezing point depression, and osmotic pressure).

Be able to use graph of solubility vs. temperature to identify a substance based on solubility at a particular temperature.

Be able to use a graph of solubility vs temperature of several substances to relate the degree of saturation of solutions to temperature.

Develop a conceptual model for the solution process.

Be able to describe the energetics of the solution process as it occurs and the overall process as exothermic or endothermic.

Be able to explain solubility in terms of the nature of solute-solvent attraction, temperature and pressure (for gases).

conductivity, and concentration.

Describe the similarities and differences among different types of solutions.

Describe the solute(s) and solvent that make up solutions.

Perform lab experiments to determine the electrical conductivity of solutions and relate it to the type of solution.

Describe how colligative properties of solutions are determined by the addition of solute and dependent upon the quantity of solute added.

Show qualitatively that all solutions posses the following colligative properties because of the addition of solutes: vapor pressure lowering, boiling point elevation, freezing point depression, and changing the osmotic pressure.

Interpret solubility curves to show the temperature that a substance is saturated, unsaturated, and supersaturated when dissolved in a given quantity of solvent (water).

Use solubility curves to determine the relative solubility of one substance compared to others as the temperature changes.

Describe and explain why some solutions release heat when they are created and some solutions absorb heat in terms of solute-solvent attraction.

Documents

Web viewUse the numbers given to me in word problems to solve the wavelength ... change during thermodynamic ... molarity of a solution given grams