Final Exam Review: Chemistry
Final Exam Review: Chemistry
Chapter 3: Properties of Matter
1. What is the difference between mass and weight? _______________________________________________
__________________________________________________________________________________________
Will your mass change or will your weight change if you go to the moon? ______________________
2. Name a fluid with high viscosity. ____________________________
Name a fluid with low viscosity. _________________________
Is viscosity a physical or chemical property? _____________________
3. What is the formula for density? _____________________________
Is density a physical property or chemical property? ____________________
4. Draw the magic circle/triangle 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?
6. What is the volume of a liquid that has a mass of 12 grams and a volume of 15 ml? ___________
If poured into water, will that liquid float or sink? ________________
7. Name two physical properties of water. ___________________________________________________
8. Identify these as physical changes (P) or chemical changes (C):
burning _____ freezing _____ grinding _____ boiling _____
9. What’s the difference between a compound and a mixture? ____________________________________
_______________________________________________________________________________________
Chapter 4: Atoms
Fill in this table:
|Sub-atomic particle |Charge |Mass ( amu) |Location in the atom |What happens if you change # |
| | | | | |
| | | | | |
| | | | | |
1. How are isotopes alike, and how are they different? _____________________________________________
_________________________________________________________________________________________
2. What does the atomic number tell you about an atom? ___________________________________________
3. What does the mass number tell you? ________________________________________________________
4. Describe Dalton’s atomic theory.
5. How many protons, neutrons, and electrons are in:
Iron-56 __________________________________________
Calcium-41 ______________________________________
29 64Cu ___________________________________________
6. What is the mass of the most common isotope of sodium? _____________ lithium? _________________
7. What part of the atom has virtually all the mass? ____________________
8. What part of the atom has virtually all the volume? ______________________________
9. What element has 15 protons in its nucleus? _____________________
10. What is the mass number of an atom that has 5 protons, 6 neutrons, 5 electrons? _________
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? ______________________________________
__________________________________________________________________________________________
3. How many electrons can fit in –
the first energy level? _______
the second energy level? ______
the third energy level? ______
4. How many valence electrons are in titanium? _________________
5. Write noble-gas configurations for the following elements:
a. cesium ___________________________
b. plutonium _________________________
6. What does an electron have to do to move to an energy level farther from the nucleus? _________________
_________________________________________________________________________________________
Chapter 6: The Periodic Table
1. What group number corresponds to these group names?
Alkaline earth metals _________________________
Halogens __________________________________
Transition metals ___________________________
Noble gases ________________________________
2. How many valence electrons do the elements in these groups have?
Group 1 ____ Group 2 _____ Group 13 _____ Group 16 _____
3. Add the correct charge to each of these ions:
Sr Na Al Ag F S O Li Zn
4. Which atoms are the smallest? ______ Which atoms are the largest? _____
5. Which element is the most electronegative? _____ Which is the least? _______
6. What is electronegativity, anyway? __________________________________________________________
__________________________________________________________________________________________
7. Why don’t the noble gases form ions? ________________________________________________________
8. As you move down a group in the Periodic Table, do the atoms get smaller or larger? __________________
Why? ______________________________________________________________________________
9. Which group of metals is most reactive? ______________________________
Which group of non-metals is most reactive? ___________________________
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:
Lithium oxide ____________________ Calcium iodide ________________________
Iron (II) nitrate ___________________ Aluminum sulfide ______________________
Ammonium nitride ________________ Strontium phosphate ____________________
Sodium carbonate _________________ Silver oxide ___________________________
Lead (IV) oxide ___________________ Copper (I) sulfate _______________________
2. Why do atoms form compounds? ____________________________________________________________
3. How does an atom form a cation? ____________________________________________________________
4. How does an atom form an anion? ___________________________________________________________
5. Name these compounds:
Fe2O3 __________________________________ CaSO4 ________________________________
AgNO3 ______________________ K2S ___________________________________
6. How many protons and electrons are in Cl_? ______________ in Be2+? _____________________________
7. Ionic bonds form between what type of elements?
Chapter 9: Covalent Compounds
1. What’s the difference between an ionic compound and a covalent compound? _______________________
________________________________________________________________________________________
2. What is a molecule? _____________________________________________________________________
3. Identify these formulas as compounds, molecules, both, or neither:
AgCl ____________________ N2O3 __________________________
I2 _______________________ AlN ___________________________
CO ______________________ NiCO3 _________________________
4. List the seven elements and the type of bond (single, double, triple) which forms that exist as diatomic molecules when they’re in the pure state. ___ ___ ___ ___ ___ ___ ___
5. Draw the Lewis structure for:
N2 Phosphate ion, PO43-
NH3 CO2
6. Name the following compounds:
a. CO ____________________________ b. CCl4 ___________________________________
c. P2O3 ___________________________ d. N2O5 __________________________________
7. When naming a compound, what do you look for to decide if it’s an ionic compound or a covalent compound? ___________________________________________________________________________
8. Name these compounds:
a. KCl ____________________________ b. SO3 ___________________________________
c. SiF4 ___________________________ d. Fe(NO3)3 ______________________________
e. AgF ___________________________ f. BiBr2 __________________________________
9. Covalent bonds form between what types of elements?
Chapter 10: Chemical Reactions
1. In a chemical formula atoms containing more than one of a particular element are designated by using __________ .
2. In a chemical equation, you balance the total number of each element on each side of the equation by using _____________________________.
3. Chemical equations can be divided into two parts: _______________________ are what you start with at the beginning of the reaction, and ________________________ are what you end up with after the reaction.
4. During a chemical reaction atoms are: ___________________________.
5. The five (5) types of chemical reactions are: ____________________ ___________________________
______________________ _______________________ ______________________.
On the above periodic table, identify the location, number of valence electrons, and ionic charge for each of the following:
alkali metals
alkaline earth metals
metalloids
halogens
noble gasses,
transition metals.
Identify the maximum number of valence electrons on each of the seven energy levels.
What is similar about elements in the same column of the periodic table?
Define the term viscosity and give two examples.
State the law of conservation of mass:
Describe how to properly read the meniscus formed in a graduated cylinder.:
Equipment identification
Properties:
|Sample/ |Luster |Conductivity |Malleability |Reaction w/acid |
|Question | | | | |
|Sample A |Dull |None |Brittle |None |
|Sample B |Shiny |Medium |Malleable |Yes |
|Sample C |Shiny |Medium |Brittle |No |
Using the above table, identify each sample as a metal, non-metal, or metalloid.
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.
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
29 64Cu p+ = 29, n⁰ = 35, e— = 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 |
| | | | |
|[pic] |[pic] | | |
| | |[pic] |[pic] |
| | | | |
2. What is correct about the Bohr model, and what is incorrect?
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
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:
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
2. Why do atoms form compounds? Trying to get full valence electrons
3. How does an atom form a cation? Give off electrons to get full valence electrons
4. How does an atom form an anion? Take on electrons to get full valence electrons
5. 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.
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:
N2 Phosphate ion, PO43-
..
:N≡N: :O:
.. | ..
: O – P – O :
.. | ..
:O:
..
NH3 CO2
.. ..
H – N – H :O = C= O:
|
H
6. Name the following compounds:
a. CO carbon monoxide b. CCl4 carbon tetrachloride
c. P2O3 diphosphorus trioxide 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 b. SO3 sulfur trioxide
c. SiF4 silicon tetrafluoride d. Fe(NO3)3 Iron III nitrate
e. AgF silver fluoride 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.
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.
Equipment identification
Graduated cylinder Flask Beaker
Properties:
|Sample/ |Luster |Conductivity |Malleability |Reaction w/acid |
|Question | | | | |
|Sample A |Dull |None |Brittle |None |
|Sample B |Shiny |Medium |Malleable |Yes |
|Sample C |Shiny |Medium |Brittle |No |
-----------------------
3
2
1
10
20
30
10
20
30
25
20
15
10
5
5
10
15
20
25
30
20
10
30
20
10
1
2
3
1 2 3 4 5 6 7 8 Valence
+1 +2 +3 +4/-4 -3 -2 -1 0 ionic charge
c charge
Alkali metals
alkaline earth metals
Transitions metals
Metalloids
Halogens
noble gasses
2
8
8
8
8
8
8
Non Metal
Metal
Metalloid
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