Name __________________________________
Final Review Answer Key
Chapter 3: Properties of Matter
1. What is the difference between mass and weight? Mass is the amount of matter in an object. Weight is
based upon the gravitational pull upon the mass.
Will your mass change or will your weight change if you go to the moon? Only weight will change.
2. Name a fluid with high viscosity. Motor oil
Name a fluid with low viscosity. water
Is viscosity a physical or chemical property? Physical
3. What is the formula for density? Density = mass/volume
Is density a physical property or chemical property? physical
4. Draw the magic circle for density.
5. What is the mass of a brick that has a density of 4.2 g/cm3 and a volume of 300 cubic centimeters?
12.6 g
6. What is the volume of a liquid that has a mass of 12 grams and a volume of 15 ml? .8 g/ml
If poured into water, will that liquid float or sink? float
7. Name two physical properties of water. Freezes at 0 ⁰ C, boils at 100 ⁰ C
8. Identify these as physical changes (P) or chemical changes (C):
burning C
freezing P
grinding P
boiling P
9. What’s the difference between a compound and a mixture? Mixtures can be separated fairly easily,
compounds cannot be separated easily.
Chapter 4: Atoms
Fill in this table:
Sub-atomic particle
Charge
Mass (in amu)
Location in the atom
Proton
+
1 amu
Nucleus
Neutron
None
1 amu
Nucleus
Electron
--
none
Electron cloud
1. How are isotopes alike, and how are they different? Have same number of protons, different number of
neutrons.
2. What does the atomic number tell you about an atom? Number of protons (number of electrons, if it is of
an element)
3. What does the mass number tell you? Number of protons and neutrons
4. Describe Dalton’s atomic theory.1. all matter composed of atoms, 2. All atoms of a given element are
identical, 3. Atoms cannot be created or destroyed, 4. Atoms combine in whole number ratios to form
compounds, 5. In chemical reaction atoms are separated, combined or rearranged.
Name __________________________________
5. How many protons, neutrons, and electrons are in:
Iron-56 p+ = 26, n⁰ = 30, e— = 26
Calcium-41 p+ = 20, n⁰ = 21, e— = 20
64
Cu p+ = 29, n⁰ = 35, e— = 29
29
6. What is the mass of the most common isotope of sodium? 23 lithium? 7
7. What part of the atom has virtually all the mass? nucleus
8. What part of the atom has virtually all the volume? Electron cloud
9. What element has 15 protons in its nucleus? phosphorus
10. What is the mass number of an atom that has 5 protons, 6 neutrons, 5 electrons? 11 amu
Chapter 5: Electrons in Atoms
1. Draw Bohr models for these atoms:
lithium
Sodium
Neon
Helium
2. What is correct about the Bohr model, and what is incorrect? It places the protons and neutrons in the
nucleus, and electrons orbiting it (where all belong). It incorrectly has the electrons orbiting in fixed
orbitals (they are actually in a cloud)
3. How many electrons can fit in –
the first energy level? 2
the second energy level? 8
the third energy level? 8
4. How many valence electrons are in titanium. 2
5. Write noble-gas configurations for the following elements:
a. cesium Xe
b. bromine Kr
6. What does an electron have to do to move to an energy level farther from the nucleus? Become excited
(take on energy)
Chapter 6: The Periodic Table
1. What group number corresponds to these group names?
Alkaline earth metals 2
Halogens 17
Transition metals 3 - 12
Noble gases 18
2. How many valence electrons do the elements in these groups have?
Group 1 1
Group 2 2
Group 13 3 Group 16 6
Name __________________________________
3. Add the correct charge to each of these ions:
Sr
Na
Al
Ag
F
S
O
Li
Zn
+2
+1
+3
+1
-- 1
-- 2
-- 2
+1
+2
4. Which atoms are the smallest? H Which atoms are the largest? Fr
5. Which element is the most electronegative? F Which is the least? Fr
6. What is electronegativity, anyway? Ability to attract electrons
7. Why don’t the noble gases form ions? They have full valence electrons
8. As you move down a group in the Periodic Table, do the atoms get smaller or larger? larger
Why? Number of protons and neutrons increases and electrons are further away from the nucleus
9. Which group of metals is most reactive? Alkali metals
Which group of non-metals is most reactive? halogens
Chapter 8: Ionic Compounds
1. Indicate the charge of the ion each element would form, and then use the criss-cross rule to find the formula
for each of these compounds:
2.
3.
4.
5.
Lithium oxide Li +1 O-2 Li2O
Calcium iodide Ca+2 I—1 CaI2
Iron (II) nitrate Fe+2 NO3 -1 Fe(NO3)2
Aluminum sulfide Al+3 S—2 Al2S3
Ammonium nitride NH4+1 N –3 (NH4)3N
Strontium phosphate Sr+2 PO4-3 Sr3(PO4)2
Sodium carbonate Na+1 CO3—2 Na2CO3
Silver oxide Ag +1 O--2 Ag2O
Lead (IV) oxide Pb+4 O –2 PbO2
Copper (I) sulfate Cu+1 SO4 -2 Cu2SO4
Why do atoms form compounds? Trying to get full valence electrons
How does an atom form a cation? Give off electrons to get full valence electrons
How does an atom form an anion? Take on electrons to get full valence electrons
Name these compounds:
Fe2O3 Iron III oxide
CaSO4 calcium sulfate
AgNO3 Silver nitrate
K2S potassium sulfide
6. How many protons and electrons are in Cl_? P+ 17 e—18 in Be2+? P+ 4 e—2
7. Ionic bonds form between what type of elements? Metal and a non-metal
Chapter 9: Covalent Compounds
1. What’s the difference between an ionic compound and a covalent compound? Ionic compounds formed
from a metal and a nonmetal which give up or take on electrons causing them to be attracted to each
other. Covalent compounds are formed by two non metals sharing electrons.
2. What is a molecule? 2 or more atoms combined together to act as 1 single unit.
Name __________________________________
3. Identify these formulas as compounds, molecules, both, or neither:
AgCl molecule
N2O3 compound
I2 molecule
AlN molecule
CO molecule
NiCO3 molecule
4. List the seven elements that exist as diatomic molecules when they’re in the pure state.
Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine
5. Draw the Lewis structure for:
NH3
Phosphate ion, PO43..
:O:
.. | ..
:O– P– O:
.. | ..
:O:
..
CO2
H–N–H
:O = C= O:
N2
:N≡N:
..
..
|
H
6. Name the following compounds:
a. CO carbon monoxide
c. P2O3 diphosphorus trioxide
b. CCl4 carbon tetrachloride
d. N2O5 dinitrogen pentaoxide
7. When naming a compound, what do you look for to decide if it’s an ionic compound or a covalent
compound? Look at the first element if metal = ionic, if nonmetal = covalent
8. Name these compounds:
a. KCl potassium chloride
c. SiF4 silicon tetrafluoride
e. AgF silver fluoride
b. SO3 sulfur trioxide
d. Fe(NO3)3 Iron III nitrate
f. BiBr2 bismuth bromide
9. Covalent bonds from between what types of elements? Non-metal – non-metal
Chapter 10: Chemical Reactions
1. In a chemical formula atoms containing more than one of a particular element are designated by using subscripts .
2. In a chemical equation, you balance the total number of each element on each side of the equation by using
coefficients
3. Chemical equations can be divided into two parts: reactants, (what you start with at the beginning of the reaction), and
products (what you end up with after the reaction).
4. During a chemical reaction atoms are: rearranged.
5. The five (5) types of chemical reactions are: synthesis, decomposition, single replacement, double
replacement, combustion.
Name __________________________________
1
2
+1 +2
c charge
3
4
5
+3 +4/-4 -3
6
-2
7
-1
8 Valence
0 ionic charge
2
8
8
8
8
8
noble gasses
Halogens
Metalloids
Transitions metals
alkaline earth metals
Alkali metals
8
What is similar about elements in the same column on the periodic table? Same number valence electrons, share
similar properties
Define the term viscosity and give two examples. Resistance of a liquid to flow. Thicker the liquid, slower it flows.
State the law of conservation of mass: Mass cannot be created or destroyed in a chemical reaction.
Describe how to properly read the meniscus formed in a graduated cylinder. Read the
bottom of the curve of the liquid. Estimate the final number.
Name __________________________________
Equipment identification
25
20
15
10
5
1
30
30
20
20
10
10
2
3
Graduated cylinder Flask
Beaker
Properties:
Sample/
Question
Luster
Conductivity
Malleability
Reaction
w/acid
Non
Metal
Sample A
Dull
None
Brittle
None
Metal
Sample B
Shiny
Medium
Malleable
Yes
Sample C
Shiny
Medium
Brittle
No
Metalloid