Chemistry Honors Multiple Choice review Name_____________________________________
Unit 1 Chapter 2 and 3 text-- Chapter 2: MATTER AND CHANGE
1.
Distinguish between a physical and a chemical change
2.
How can you know that a chemical change occurs?
3.
Distinguish between an intensive and an extensive property
4.
Complete the following chart:
Property
1.Wood burns in air
Physical or chemical Intensive or extensive
2. Freezing point
3. Silver tarnishing
4. Silver nitrate and sodium chloride form a precipitate
5. volume
6. mass
5.
Distinguish between a mixture and a pure substance
6.
Distinguish between a homogeneous and heterogeneous mixture
7. In a mixture a phase is _________________________________________________________
How many phases does :a) a salt water solution have? b) a mixture of salt and pepper have?
8. How do you Distinguish between an element and a compound
7. Classify the following as either a homogeneous or heterogeneous mixture, a compound, or an element a. Diamond (made up of only carbon)__________________ b. water___________________ c. Salt water solution _____________________ d. air___________________________
e. chicken noodle soup ____________________ f. gold_____________________________
1

CHAPTER 3 Text
1.
How many significant digits are there in:
120 0.00120
1.04 x 10
4
6.012 x 10
9
0.0000012
2.
Distinguish between accuracy and precision
3.
If the mass of a piece of aluminum is 4.55 g and its actual density of Al is 2.70 g/cm
3
, then what is its volume?
4. Write the name and the exponential meaning of the metric prefixes used in this chapter
UNIT 2 THE ATOM__Chapter 4 and 5 of text
CHAPTER 4
1.Define atom
2. Describe the contributions to atomic theory in detail made by each of the following
Dalton
Thomson
Rutherford
Bohr
3. Describe each subatomic particles in terms of their location, relative mass, and charge
Proton
Neutron
Electron
2

4.Which subatomic particle determines the identity of an atom?______Which determines which isotope?_________
5. The nuclear symbol of the tritium isotope of hydrogen is 3
1
H. What do the numbers in the nuclear symbol indicate?
6.
. Define atomic number, mass number and atomic mass.
7.
Use you periodic table to Fill in the table below
Symbol
14
6
C
Ca
Ca +2
Atomic number
Atomic
Mass
Mass number
Protons Neutrons Electrons name
CHAPTER 5- ARRANGEMENT OF ELECTRONS IN ATOMS
1.An electron in its lowest energy state is in the _______________state
2.
The movement of an electron from its ground state to an excited state occurs when an atom absorbs__________, and when the electron drops back down to the ground state, it gives off _____
3.
What color of visible light has the smallest wavelength? _____ Which color has the longest wavelength?__________________________ Which type of electromagnetic radiation has the longest wavelength? ___________ the shortest wavelength? ___________-The highest frequency?
_____________________The lowest frequency? _____________________
3

4.
Frequency and Wavelength are _______________________proportional.
5.
Frequency and energy are __________________________ proportional
6.
What is the mathematical formula that allows you to calculate the energy of a photon if you know its frequency?
7.
What is the aufbau principle?
8.
Fill in the following chart:
Energy level
(n)
1
Total # sublevels (list them)
# orbitals Number of electrons
2.
3.
4.
9.
What does the principle quantum number tell you about an atom?
10.
An orbital is where there is a high ______________________ of finding an electron.
11.
How many different s orbitals are there in an s sublevel?
12.
How many different p orbitals are there in an p sublevel?
13.
How many different d orbitals are there in an d sublevel?
4

14.
How many different f orbitals are there in an f sublevel?
15.
Which is the next highest energy orbital after 4f? __________________
16.
Which element has an electron configuration of 1s 2 2s 2 2p 6 3s 1? __________
17.
What is the maximum number of electrons that can be found in the following energy levels:
1st____________ 2nd____________ 3rd____________ 4th _______________
18.
The fourth energy level of an atom with n=4 contains how many different sublevels
19.
______________________states that no 2 electrons in the same atom have the same 4 quantum numbers
20.
Write the orbital notation of oxygen below. How many half-filled sublevels does oxygen have?
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UNIT 3-- THE PERIODIC Table--Chapter 6 text
3.
Fill in the table below
6

4.
What happens to an atom when it forms a cation?
5.
What happens to an atom when it forms an anion?
UNIT 4-- MOLECULAR COMPOUNDS/BONDING--Chapter 8 text
1.
For each of the following, draw the Lewis Structure, and then indicate the molecular geometry
(shape) a.NH
3
____________________ d.SF
6
____________________ b.PCl
5
____________________ e.SBr
2
____________________ c.SiCl
4
____________________ f. OCl
2
____________________
2. For each molecule listed above, determine of the molecule is 1)polar or nonpolar and 2) identify its intermolecular force a. 1. d. 1.
2. b. 1.
2.
2. e. 1.
2. c. 1.
2. f. 1.
2.
3. Which intermolecular force is the strongest? ___________ Which is the weakest??________
4. For each molecule above, put them in order from the lowest to the highest boiling points:
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Unit 5 Formula naming and writing. and Chemical quantities Ch 9 and 10 text
Write the correct formula or name the following compounds
1.
magnesium sulfide
2.
CO
3.
MgCl
2
4.
Na
2
HP0
4
5.
H
2
CrO
4
6.
SbBr
3
7.
Na
2
SO
4
16.
17.
18.
19.
20.
21.
22.
potassium carbonate hydrosulfuric acid potassium sulfate silver sulfide strontium hypochlorite phosphorus pentachloride sodium sulfate
8.
Na
2
C
2
O
4
9.
H
3
PO
3
10.
Na
3
PO
4
11.
NaOH
12.
Ni
2
(SO
3
)
3
13.
nitrous acid
14.
Pb(NO
3
)
4
23.
24.
25.
26.
27.
28.
29.
mercuric thiocyanate lithium bisulfite
Sr(NO
3
)
2 sulfurous acid strontium phosphide zinc chlorate zinc hydroxide
15.
PbO
2
30.
carbon tetrachloride
2. Calculate the molar mass and percent composition of zinc hydroxide
3. Calculate the grams of zinc hydroxide needed to make 500. ml of a 2.25 M solution of Zinc hydroxide
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4a. Find the empirical formula of Ascorbic acid which contains 40.92% C, 4.58% H and 54.50 %O by mass. b. If its molecular mass is 176.2, what is its molecular formula?
5. What is Avogadro's number?
UNIT 6 CHEMICAL EQUATIONS
: Classify each reaction, use solubility chart and activity series to predict if reaction will occur And write the correctly balanced chemical equation
_________1) Aqueous aluminum nitrate is reacted with a piece of magnesium
___________________________________________________________________________________
________2) Solid potassium chlorate is decomposed
___________________________________________________________________________________
_______3) Aqueous solutions of sulfuric acid and magnesium hydroxide react
___________________________________________________________________________________
______4) a piece of Iron reacts with oxygen gas (assume ferric in product)
___________________________________________________________________________________
_____5) Solid nickel II carbonate decomposes
___________________________________________________________________________________
______6) Aqueous magnesium bromide is reacted with fluorine gas
___________________________________________________________________________________
______7) Solid calcium oxide and carbon dioxide react
9

___________________________________________________________________________________
______8) butane gas (C
4
H
10
) is combusted (don’t forget oxygen is a reactant!)
___________________________________________________________________________________
______9) Solid calcium chlorate decomposes
___________________________________________________________________________________
______10) Aqueous solutions of sodium phosphate and lead II nitrate react
___________________________________________________________________________________
_____11) Solid strontium chloride reacts with oxygen gas to form a solid product
___________________________________________________________________________________
_____ 12) A piece of aluminum is placed in a solution of lithium chloride
___________________________________________________________________________________
UNIT 7 STOICHIOMETRY
1. 15.00 g of Zn is combined with 40.00 g of HCl in a single displacement reaction.
A)What is the limiting reagent
B) How much of each product will be produced?
C )What is the excess reagent?
D)How much excess reagent is left?
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UNIT 8 GAS LAWS
1. Write the equations for the following:
a. Boyle's Law
b. Charles' Law
c. Gay-Lussac's LAw
d. Combined gas law
2. The molar volume of a gas is = __________________
3. When using temperature in a gas law, the temperature must be expressed in ___________________
4. At STP, temperature= _______________ and pressure = ________________
4. Distinguish between diffusion and effusion
5 5.00 L of a gas at 45 o C and 5.05 atm is heated to 60 o C and the pressure is reduced to 2.55 atm.
Calculate the new volume.
6. A 5 L of a gas is at 22 C and 0.75 atm pressure. How many moles of this gas is present? (R= 0.0821 L atm/mol K)
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