Name:_______________________________________

Mid term review sheets for Chemistry Due:_______________________________________

Atomic Structure

Define the following terms

Rutherfords Experiment : Gold Foil Shot alpha particles at gold foil and some bounce back most went through Atom is mostly empty space with a dense positive center.

Nucleons: particles in the nucleus, protons and neutrons

Mass Number: protons plus neutrons found on periodic table in the upper left corner

Ground State: Lowest energy state of an electron found on the periodic table under the element

Spectroscope: Device used to see spectral line

Excited State: When electron gets excited it jumps to a higher energy level called the excited state

Spectrum: light given off when electrons return to the ground state from the excited state

Atomic Number: number of protons, found in the lower left corner of the periodic table.

Orbitals: area of probable location of an electron from the modern theory

Isotope: Elements having the same number of protons, different neutrons or atomic mass

Energy Levels : areas where electrons are found. Electrons in higher energy levels have more energy

Answer the following questions in complete sentences.

1. Why is the atomic mass a decimal and not a whole number?

It is an average of all the naturally occurring isotopes

2. How do you determine the atomic mass of an element if you are given the relative abundance of all of its naturally occurring isotopes?

(mass)(%)/100 + (mass)(%)/100+ ….

Mass(% converted to decimal) + Mass (% converted to decimal) …

3. Draw the electron configuration, mass, atomic number, protons, neutrons, electrons and electron dot diagrams for the first 18 elements. This is the official answer sheet.

Element Electron configuration

Mass AtomicNumber

Protons Neutrons Electrons Electron dot digram

H

He

Li

Be

B

C

N

O

F

Ne

Na

Mg

Al

Si

P

S

Cl

Ar

Nuclear Chemistry

Define the following terms: These are the answers that were on the smart board

Beta Decay: When a unstable nucleus gives off a beta particle, go toward the Positive plate in an electric field. Moderatly penetrating

Radioactivity: when an unstable nucleus breaks down and gives off radiation. Any element over number 82 is radioactive.

Gamma Radiation: high energy with no mass and charge

Transmutation: changing of one element into another element by releasing energy

Half life: the amount of time it takes for half of a radioactive isotope to decay to another isotope

Alpha Decay : when an unstable nucleus gives off an alpha particle.

1= fission 2= fusion 3= artificial transmutation 4= natural transmutation

Answer the following questions in complete sentences.

List the radioisotopes and uses1. Carbon-14: dating living things2. U-238: date rocks3. I-131: thyroid4. Co-60: cancer 5. Fe:59: blood disorders 6. Tc-99: brain tumors7. P-32: plant studies

What are the advantages and disadvantages to fission.

Matter and Energy

Define the following: Remember some of these are not on your test Tuesday but we will do wednesday

Matter: Anything that has mass and takes up space. Can be divided into substances or mixtures

Heterogeneous mixture: unevenly mixed. Can be physically separated

Element: found on the periodic table. Cannot be physically or chemically separated

Compound: 2 or more elements combined in fixed proportions. Can be chemically separated

Homogeneous Mixture: evenly mixed. Also called a solution also called aqueous mixture (aq)

Kinetic Energy: energy of motion; directly related to temperature

Conservation of Energy: energy cannot be created or destroyed just changes forms.

Absolute Zero: 0Kelvin, motion stops

Boiling: when vapor pressure equals atmospheric pressure. Table H. High vapor pressure easier it is boil. Strong intermolecular forces harder to boil.

Crystalizing: liquid to solid

Potential Energy: stored energy in bonds or position

Normal Boiling Point: 100C and 373 K at STP

Melting Point: when solid changes to liquid

Sublimation: solid to gas ex dry ice (carbon dioxide) and iodine

Evaporation: liquid to gas

Exothermic : releases heat, Cooling curve

Endothermic: absorbs heat. Heating curve

Answer the following questions in complete sentences.

1. What are the 2 fixed points on a thermometer in Celsius and Kelvin?

2. Describe and draw a particle diagram for solids, liquids and gases.

3. Draw an exothermic and endothermic heating /cooling curve and label all phases, changes in kinetic and potential energy and relevant points.

Periodic TableDefine the followingIonization Energy: energy needed to remove a valence electron found on table SElectronegativity: desire for more electrons found on table S. Tells you polarity Higher electronegativity is the (-) of the molecule.Atomic Radius: half the distance between the nucleus and the outer electrons found on table sValence Electrons: last shell of electrons responsible for bonding and found in Lewis dot diagramsPeriod: horizontal row the tells the energy level being filledGroup: vertical column that tells valence electrons and have similar properties

Answer the following questions in complete sentences.

1. Describe the trends in Atomic Radius, Ionization Energy and Electronegativity as you go across a period and down a group on the periodic table.

2. Why do elements in the same group have similar bonding and reactivity?

Same valence electrons

3. Compare the ionic and atomic radius of metals and non metals.

Metals Atomic radius > ionic radius

Nonmetals Atomic radius < ionic radius

4. What are the only liquids on the periodic table?

Mercury and Bromine

5. What are the only gases on the periodic table?

Hydrogen, Helium, Nitrogen, Oxygen, Fluorine, Chlorine, Neon, Argon, Krypton, Xenon, Radon

6. Who are the metalloids?

Boron, Silicon, Arsenic, Germanium, Antimony, Astatine, Tellurium,

7. Why are the transition metals different?Colored Solutions

Bonding

Define the following

Ionic bond: Metal and nonmetal. Transfer of electrons from the metal to the non metal.

High melting points, conduct electricity when dissolved in water, hard

Covalent bond: sharing of electrons between non metals

Low melting point, never conduct, soft

Molecular substance: covalent substance

Van der Waals forces: weak intermolecular forces between non polar molecules, Increase as molecules get larger

Polar bond: unequal sharing of electrons. Higher electronegativity is the negative side BEND

Polar molecule; non symmetrical SNAP

Non polar bond: Br, I, N,Cl, H O, F even sharing, nitrogen and carbon triple bonds (6 electrons) oxygen and carbon double bonds (4 electrons)

Non polar molecule: symetrical

Metallic bond: sea of mobile electrons which is why metals conduct electricity

Dipoles: polar molecules

Hydrogen bonds: intermolecular forces that create high boiling points in molecules when hydrogen bonds to nitrogen, fluorine or oxygen

Answer the following questions in complete sentences.

1. How do polar bonds and polar molecules differ?

Polar bonds are different elements, polar molecules are not symetrical

2. What elements have both non polar bonds and molecules?Bromine, Iodine, Nitrogen, Chlorine, Hydrogen, Oxygen and Fluorine

3. Draw the following and give their shape and polarity

N2 CO2 H2O AlCl3 O2

4. Name the followinga. NaCl: Sodium Chloride

b. CuCl: Copper (I) Chloride

c. KMnO4: Potassium Permanganate

d. CO2: Carbon Dioxide/ Carbon (IV) Oxide

5. Write the formula for the following:

a. Iron (III) Oxide: Fe2O3

b. Lithium Chloride: LiCl

c. Dinitrogen Pentoxide: N2O5

Math and Equations

Balance the following

_____ Na2CO3 + _____ H3PO4 → _____ Na3PO4 + _____ H2O + _____ CO2

_____ H2SO4 + _____ NaOH →_____ Na2SO4 + _____ H2O

_____ Sn + _____ P4 → _____ Sn3P4

_____ H2O → _____ O2 + _____ H2

_____ C4H8O + _____ O2 → _____ CO2 + _____ H2O

_____ AgMnO4 + _____ Sr → _____ Ag + _____ SrMnO4

Calculate the gram formula mass for the followingCuNO3 *3H2O Cu3(PO4)2

Calculate the percent oxygen in Cu3(PO4)2

Calculate the percent water in CuNO3 *3H2O

How many moles of CuNO3 *3H2O are there in 300 grams?

How many grams are there in 3.2 moles of CuNO3 *3H2O?

If a molecule has a molecular mass of 45 and an empirical formula of CH3. What is its molecular formula?

How many moles of Nitrogen are needed to make 16 moles of Ammonia (NH3) using the balanced equation below

N2 + 3H2 2 NH3

Honors: How many grams of Hydrogen are needed if 72 grams of nitrogen are used to make ammonia?