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Honors Chemistry Final Review

Total questions: 50

Worksheet time: 29mins

Name
Class
Date
1.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
2.

When an atom loses electrons, it is...

a)

a positively charged cation

b)

a positively charged anion

c)

a negatively charged cation

d)

a negatively charged anion

3.

Which temperature scale is used to measure the temperature of a gas?

a)

Celsius

b)

Kelvin

c)

Fahrenheit

d)

Any temperature scale can be used

4.

Which pair of atoms will form ionic bonds?

a)

S and F

b)

Mg and O

c)

F and Cl

d)

H and Ne

5.

How many atoms are there in one mole of any element?

a)

6.02x10-23

b)

6.02x1023

c)

22.4

d)

2.06x10-2

6.

What is the mass in grams of 3.50 moles of boron?

a)

2.11x1024 grams

b)

37.8 grams

c)

0.324 grams

d)

3.09 grams

7.

How does increasing the pressure on a gas impact the volume of the gas?

a)

volume would decrease proportionally

b)

volume would increase proportionally

c)

volume would become zero

d)

it is impossible to predict the relationship between pressure and volume

8.

Describe the relationship between the temperature and pressure of a gas.

a)

Directly proportional

b)

Inversely proportional

c)

Exponential

d)

There is no predictable relationship

9.

In an endothermic reaction, heat is

a)

absorbed

b)

released

10.

Calculate the molarity of 0.212 mol of KBr dissolved in 0.750 L.

a)

0.280 M

b)

0.210 M

c)

33.3 M

11.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
12.

Determine the number of significant figures in the measurement 5.6 x 108 km.

a)

1

b)

2

c)

10

d)

8

13.

What is the correct name for the compound Ca(NO3)2?

a)

Calcium nitrite

b)

Calcium mononitrogen trioxide

c)

Calcium Dinitrate

d)

Calcium nitrate

14.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
15.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
16.

How many valence electrons does Chlorine have?

a)

5

b)

2

c)

7

d)

8

17.

What is matter?

a)

Anything that has mass and takes up space

b)

How dense an object is

c)

The amount of space an object takes up

d)

The transfer of heat through the rising and falling movement in a gas or a liquid in which the warmer parts rise and colder parts sink

18.

Which element has the greatest ionization energy and electronegativity?

a)

fluorine

b)

chlorine

c)

bromine

d)

iodine

19.
Based on their locations in the periodic table, which element has chemical properties most similar to those of calcium, Ca?
a)
beryllium, Be
b)
potassium, K
c)
titanium, Ti
d)
yttrium, Y
20.
According to kinetic-molecular theory, particles of an ideal gas
a)
attract each other but do not collide
b)
repel each other and collide
c)
neither attract nor repel each other but collide
d)
neither attract nor repel each other and do not collide
21.
What is the order of strength of intermolecular forces from weak to strong?
a)
dipole-dipole, dispersion, hydrogen
b)
hydrogen, dispersion, dipole-dipole
c)
dispersion, dipole-dipole, hydrogen
d)
hydrogen, dipole-dipole, dispersion
22.
Given the reaction: 4Al + 3O2 --> 2Al2O3
How many moles of Aluminum oxide do you have if you have 2 moles of Al?
a)
3 mole
b)
2 mole
c)
1 mole
d)
0.5 mole
23.

What product forms in this reaction?


HNO3 + LiOH --> __________ + H2O

a)

LiNO3

b)

LiH2O

c)

NO2

d)

LiO3

24.

What is the relationship between wavelength and frequency of all waves on the electromagnetic spectrum?

a)

Wavelength and frequency are directly related.

b)

Wavelength and frequency are inversely related.

c)

Wavelength and frequency are unrelated.

d)

Wavelength and frequency are equal.

25.

Which of the following is a property of metals?

a)

They generally have low melting points.

b)

They are all liquids at room temperature except mercury.

c)

They are bad conductors of heat and electricity.

d)

They are malleable & ductile

26.

Chemical equations must be balanced to satisfy ____.

a)

The law of definite proportions

b)

The law of multiple proportions

c)

The law of conservation of mass

d)

Avogadro's principle

27.

What is the name of H2SO4?

a)

hyposulfuric acid

b)

hydrosulfuric acid

c)

sulfuric acid

d)

sulfurous acid

28.

The equation 2C3H7OH + 9O2 → 6CO2 + 8H2O is an example of which type of reaction?

a)

Combustion reaction

b)

Single replacement reaction

c)

Double replacement reaction

d)

Decomposition reaction

29.
Which state of matter is represented here?
a)
Solid
b)
Liquid
c)
Gas
30.
What kind of intermolecular force is shown here?
a)
hydrogen bonding
b)
London dispersion
c)
network covalent
d)
electrostatic (ionic)
31.
2.   Which of these recorded observations is qualitative, rather than quantitative?
a)
a.  A chemical reaction is complete in 2.3 s.
b)
a.  The solid has a mass of 23.4 g.
c)
The compound melts at 87.5°C.
d)
Iron is denser than aluminum.
32.
3.  A sample of bismuth has a mass of 343g and a volume of 35.0cm3. What is the density of bismuth?
a)
a.  0.102 g/cm3 
b)
b. 9.80 g/cm3 
c)
c. 378 g/cm3 
d)
d. 1.20 x 104 g/cm3
33.
7.  Convert the following measurement:  5.4 L to mL
a)
54. mL
b)
5400. mL
c)
540. mL
d)
54000. mL
34.
9.  What electron configuration rule states: All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Pauli Exclusion Principle
b)
Hund's Rule
c)
Aufbau Principle
d)
Bohr Model of the the atom
35.
17. Which coefficients correctly balance the formula equation below? KClO3 (s)---> KCl(s) + O2(g)
a)
1,1,1
b)
1,1,3
c)
2,2,3
d)
2,1,1
36.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
37.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
38.

Magnesium can be burned in oxygen to produce solid magnesium oxide. (Ignore balancing for this question)

a)

Mg(s) + O2(g)→ MgO(s)

b)

Mg(s) + O(g) → MgO(s)

c)

Mg(s) + CO2(g) → MgO(s) + C(s)

d)

Mg(s) + O2(g) → Mg2O2(s)

39.

An atom of an element has 9 protons, 11 neutrons, and 10 electrons. Which of the following facts is false?

a)

The element is fluorine.

b)

The atomic number is 9.

c)

The mass number is 19.

d)

The charge is -1.

40.

Determine the charge for an ion that has 33 protons, 36 electrons, and 38 neutrons.

a)

+3

b)

-3

c)

+5

d)

-5

41.

Potassium-42 has a half-life of 12.4 hours. How much of an 848 g sample of potassium-42 will be left after 62.0 hours?

a)

5 g

b)

424 g

c)

170 g

d)

26.5 g

42.

Determine the missing isotope.

a)

thorium-238

b)

uranium-238

c)

curium-246

d)

silver-121

43.

Which type of radiation has no mass and no charge?

a)

alpha

b)

beta

c)

gamma

44.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

Ethane (C2H6) combusts (burns) in the above reaction. What is the mole ratio of ethane to oxygen gas?

a)
b)
c)
d)
45.

Choose the one that is a chemical property

a)

Magnetism

b)

Size

c)

Color

d)

Reactivity with water

46.
What type of mixture is this?
a)
homogenous mixture
b)
chemical
c)
heterogeneous mixture 
d)
solid mix
47.

What is the name of group 1 on the periodic table

a)

Alkaline Earth Metals

b)

Boron Family

c)

Alkali Metals

d)

Halogen Family

48.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
49.
As the wavelength of light increases
a)
the frequency increases.
b)
the speed of light increases.
c)
the energy decreases.
d)
the intensity increases.
50.

Which of the following measurements contains three significant figures?

a)

0.030

b)

0.300

c)

3.00

d)

0.0030

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