Distinguish between chemical and physical changes and properties Know the states of matter and characteristics of each Understand the difference

Chapter 1 : Learning Targets

Distinguish between chemical and physical changes and properties Know the states of matter and characteristics of each Understand the difference between elements, molecules,

compounds, and mixtures. Know the various techniques for separating the components of a

mixture, and the principle upon which each of these operates Be familiar with the units of the metric system and the

temperature scales

Understand the concept of density and be able to answer all questions, both conceptual and mathematical, related to density

Be able to convert measurements, especially within the metric system, by using dimensional analysis

Determine the number of significant figures in a measurement and be able to express the results of a calculation with the proper number of significant figures

Chapter 2: Atoms, Molecules, and Ions

Understand the atomic theory, and how it relates to theories of chemistry Distinguish between protons, neutrons, and electrons, and be able to

describe the composition of an atom of any particular element in terms of these subatomic particles

Understand the difference between isotopes, as well as the two types of notations used with them

Be aware of who discovered each subatomic particle and have an idea of how they did it

Know the difference between an atom, and ion, and a molecule Have a basic knowledge of the periodic table, which includes being able

to predict whether an element is a metal or a nonmetal, and what will be the probable charge of its ion

Know that the given atomic mass of an element is the weighted average of the atomic masses of all isotopes of that element. Be able to perform all related calculations

Be able to give the name and/or formula for any given compound

Key Words: Chapter 1 Matter

Molecule Distillation Pure substance Compound Solution Physical properties Intensive properties Physical change Density

Atom Filtration Chromatography Element Mixture Chemical properties Extensive properties Chemical change Significant Figures

Key Words: Chapter 2 Atom

Ion Proton Neutron Electron Atomic number Nuclide Group Period Anion

Molecule Isotope Mass Number Atomic Weight Metal Nonmetal Metalloid Molecular Formula Empirical Formula Cation

Section 1: Separation TechniquesPages 11-12 RBQs # 15,16,78,79

A mixture is a combination of two or more substances in which each substance retains its own chemical identity

Because they retain their chemical identities, a mixture can be separated by physical means, as opposed to a compound

Three common means of separating mixtures are filtration, distillation, and chromatography


Filtration:


Distillation:


Paper Chromatography:


Gas Chromatography :

Section 2: Units & Measurement Pages 13-17 RBQs # 19-25,29,30

Lab data can be either quantitative or qualitative

Qualitative:

Quantitative:


Quantitative data (measurements) MUST include a number and unit

The units in chemistry are called the SI Units; these are the internationally agreed upon set of units


The SI base units are modified using metric prefixes to make the number more manageable


You won’t use these, but they are too awesome to leave out:



The instruments used to make measurements have limitations which leads to estimations being made


When a measurement is made, all certain digits are recorded, and the final estimated digit is uncertain digit

Every measurement will contain all certain digits and one estimated uncertain digit; combined, these digits are known as the significant figures

To make sure the proper number of digits is reported, and therefore the uncertainty of the result is known, the rules of significant figures are applied to numbers and calculations


How many significant figures are in the measurement 4.003

m?A. 0B. 1C. 2D. 3E. 4

How many significant figures are in the number 6.023 x 1023?

A. 0B. 1C. 2D. 3E. 4

How many sig figs are in the number 5000?

A. 0B. 1C. 2D. 3E. 4



Do this! 1.05 x 10-3 ÷ 6.135 =

A. 1.71 x 10-4

B. 1.7 x 10-4

C. 2 x 10-4

D. 1.711 x 10-4

E. 1.71149144 x 10-4

Do this! 21- 13.8 =A. 7.20

B. 7C. 7.200D. 7.0E. 7.2

9.5 + 4.1 +3.1754

A. 4.19375B. 4.194C. 4.2D. 4


An important technique for problem solving is called dimensional analysis which uses conversion factors

This technique is used to convert a quantity to an equivalent quantity, but with a different unit

For example, dimensional analysis could show 3 dollars are equal to 12 quarters; same amount of money, yet different units


The first thing to know is the numerical relationship between the starting quantity and the desired quantity

For example, if the number of meters in a given number of inches is needed, one must know the number of inches in a meter (or vice versa)

There are 39.37 inches in 1 meter, and as a conversion factor, this information could be written as seen below:


The conversion factor will always be a fraction, and once it is determined, the conversion factor is arranged so that the given unit is eliminated and replaced with the desired unit

For example, if the questions wants to know the number of meters in 69.5 inches:

A pencil is 7.000 in long. What is this length in cm? (1 in = 2.54 cm)

A. 20B. 18C. 17.7D. 17.8E. 17.78

A N2 molecule moves at 515 m/s. What is this in mi/hr?

A. 1152B. 1150C. 1152.2D. 1152.23E. 115

Section 3: Atomic Structure & MassPages 35-45 RBQs # 13-21,23,24

The atom is the basic building block of matter; it is defined as the smallest unit of an element that retains the properties of that element

→ An atom of gold is the smallest piece of gold that is yellow and shiny→ An atom of oxygen is the smallest unit of oxygen that we can breathe

The concept of the atom has been around for thousands of years, but this idea has only been backed by scientific experimentation since the 1700’s

The atom’s existence and structure was confirmed and determined through a number of experiments by several scientists


All matter is composed of extremely small particles called atoms

Atoms of a given element are identical

Atoms cannot be created, destroyed, or divided

Atoms combine in whole number ratios to form compounds

In chemical reactions, atoms are separated, rearranged and combined

John Dalton.Smart, but not always right.


J.J. Thompson did most of the heavy lifting in the discovery of electrons with the cathode ray tube


Ernest Rutherford was all up in the nucleus with the gold foil/alpha particle experiment


Another thing learned through all this research was that all atoms of a given element do not have the same mass

Isotopes are atoms of a given element that have different masses; the difference in these masses results from different numbers of neutrons

An atom of a specific isotope is called a nuclide


These different nuclides are detected and counted using a technique called mass spectrometry which can be used to identify unknowns and determine atomic masses


The result is a mass spectrum such as this:

23

100


The y-axis will have a scale that can be read, but let’s just let the computer give us the numbers

Based on the height of each peak, the amount of each isotope/nuclide in the sample is determined

The spectrum above shows 100 nuclides with a mass of 11 and 23 nuclides with a mass of 10


This information can also be given as percentages

23

100

Section 4: Periodic Table, Molecules, IonsPages 46-56 RBQs # 29-32,36-38,41-50

The elements are arranged by increasing atomic number in groups and periods, and also by element type (metal, nonmetal, metalloid)


The real fun starts when elements combine to form compounds

Sometimes these compounds are called molecules


Once metals get involved, we have ionic compounds


Ion charges can be predicted using the periodic table

Section 5: Chemical NomenclaturePages 56-65 RBQs # 51-66

Determining the names and formulas of a chemical compound is kind of a big deal in chemistry

There are four types of compounds that each have their own rules when it comes to nomenclature

Ionic compounds, covalent/molecular compounds, acids, and organic compounds


For ionic compounds, just give the name of each ion, with the cation always first

The name of monatomic cation is the same as the element

The only exception is when the monatomic cation can have multiple charges, like most transition metals


The name of monatomic anion keeps the same base as the element , but the ending changes to –ide

The name of a polyatomic ion never changes

Name this! K2SO4

A. Potassium SulfideB. Potassium SulfiteC. Potassium SulfateD. Potassium(I)

Sulfate

Name this! Ba(OH)2

A. Boron HydroxideB. Barium HydroxideC. Barium(II)

HydroxideD. Baryllium

Hydroxide

Name this! FeCl3A. Iron ChlorideB. Iron TrichlorideC. Iron(II) ChlorideD. Iron(III) Chloride

Formula This! Ammonium Sulfide

A. (NH4)2SO4

B. (NH3)2S

C. NH4S

D. (NH4)2S

Formula this! Cobalt(II) Nitrate

A. Co(NO3)2

B. Cu(NO3)2

C. Co2NO3

D. Co3N2

Formula This! Chromium(III) Oxide

A. Ca2O3

B. Cr3O2

C. CrOD. Cr2O3


Binary covalent compounds are named using prefixes to indicate the number of each element present in each molecule

The name of the compound always ends in –ide The prefix mono- is never used with the first element

Name This! SO2

A. Sulfur(IV) OxideB. Sulfur DioxideC. Monosulfur

DioxideD. Sulfur Oxide

Name This! Cl2OA. Dichlorine

MonoxideB. Dichlorine OxideC. Chlorine(I) OxideD. Dichlorine(I)

Monoxide

Formula This! Phosphorus Pentachloride

A. PCl5B. P5Cl

C. PClD. FCl5

Formula This! Dinitrogen Tetroxide

A. N4O2

B. NOC. NO2

D. N2O4


Acids are identified because their formula begins with an H (in most cases) or the name contains the word ACID (in all cases)

Acid naming is all about the anion (the part that isn’t H)

HCl HNO3 HC3H3O2

Anion ends in –ide = hydro-_________-ic acid

Anion ends in –ate = acid name ends with “–ic acid”

Anion ends in –ite = acid name ends with “-ous acid”

Name This! H2SO3

A. Hydrosulfuric AcidB. Sulfurous AcidC. Sulfuric AcidD. Hydrosulfurous

Acid

Name This! HCNA. Cyanic AcidB. Cyanous AcidC. Hydrocyanic

AcidD. Hydrocyanous

Acid

Formula This! Hydroselenic Acid

A. H2OSe

B. HSeO2

C. HSeD. H2Se

Formula This! Phosphorous Acid

A. H3P

B. H3PO4

C. H3PO3

D. HPO3


The name of an organic compound depends on its base alkane

Alkanes are compounds made of C and H with all single bonds


Other classes of compounds are obtained when 1 or more H’s in an alkane are replaced with function groups

Alcohols are obtained when an H is replaced with an –OH; this changes the ending of the alkane to -ol


Aldehydes and ketones are obtained when an H is replaced with a double-bonded oxygen (= O)

Aldehydes have the double-bonded oxygen (= O) on a terminal carbon, ketones have it on an interior carbon

Aldehyde names end with –al, Ketone names end with -one


Carboxylic acids take a terminal C and make it a –COOH

The ending of the alkane becomes –oic acid


Alkenes and Alkynes result from the presence of double or triple bonds

Alkenes have a double bond and end in –ene Alkynes have a triple bond and end in -yne


A number indicates the carbon on which a function group is found

The carbons are always numbered to put the functional group on the lowest numbered carbon possible

2-pentanone

Formula This! 2-pentanol

A. C3H7OH

B. C5H12OH

C. C4H9OH

D. C5H11OH

Formula This! Propanoic Acid

A. CH3COOH

B. C2H5COOH

C. HCOOHD. C3H7OH

Formula This! 2-hexanone

A. C6H12O

B. C7H14O

C. C6H13OH

D. C5H11COOH

Formula This! Ethanal

A. C2H5OH

B. C2H4O

C. C3H7OH

D. C3H6O

Documents

Distinguish between chemical and physical changes and properties Know the states of matter and characteristics of each Understand the difference