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Chemistry Midterm Review

Total questions: 83

Worksheet time: 2hrs 15mins

Name
Class
Date
1.

In an atom, an orbital represents

a)

the most probably location of a proton

b)

the most probable location of an electron

c)

the least probably location of a neutron

d)

photons emitted as electrons move to lower energy levels

2.

Which particle has a mass so small, it is considered to be 0 amu?

a)

proton

b)

hydrogen nucleus

c)

neutron

d)

electron

3.

What quantity is the same among atoms of the same element?

a)

mass number

b)

atomic number

c)

number of neutrons

d)

number of nucleons

4.

An atom that has 8 protons and 10 neutrons is an isotope of the element

a)

nitrogen

b)

oxygen

c)

fluorine

d)

neon

5.

Which elements have the most similar chemical properties?

a)

Ge, As, and Sb

b)

Mn, Fe, and Co

c)

S, Se, and Te

d)

P, S, and Cl

6.

Which atom has the lowest electronegativity?

a)

Nitrogen

b)

Oxygen

c)

Fluorine

d)

Neon

7.

What is the overall charge of an ion that has 9 protons, 11 neutrons, and 10 electrons?

a)

+1

b)

-1

c)

+2

d)

-2

8.

Which electron configuration represents the atoms of a bromine atom in the excited state?

a)

2-8-18-7

b)

2-8-18-8

c)

2-8-17-8

d)

2-8-18-7-1

9.

Which formula represents a polar molecule?

a)

Cl2

b)

CH4

c)

HCl

d)

CO2

10.

Which compound has both ionic and covalent bonds?

a)

CH4

b)

CO

c)

CaCl2

d)

MgSO4

11.

As the elements in Group 2 in the periodic table are considered in order of increasing atomic number, there is a general increase in

a)

stability

b)

atomic radius

c)

electronegativity

d)

first ionization energy

12.

How many electron pairs are shared between the atoms in an N2 molecule?

a)

1

b)

2

c)

3

d)

4

13.

How would you classify NaCl?

a)

element

b)

compound

c)

heterogeneous mixture

d)

homogeneous mixture

14.

Which pair of atoms will form ionic bonds?

a)

S and F

b)

Mg and O

c)

F and Cl

d)

H and Ne

15.

What are 3 examples of metals:

a)

Lithium

Sodium

Calcium

b)

Nitrogen

Oxygen

Fluorine

c)

Helium

Neon

Argon

16.

What is the correct Lewis dot structure for Selenium:

a)
b)
c)
17.

Why is the image the correct Lewis dot for Selenium?

a)

It is in group 1, with 1 valence electron

b)

It is group 2, with 2 valence electrons

c)

It is in group 16, with 6 valence electrons

18.

Which element is this Bohr diagram from?

a)

Selenium, because it has 34 electrons

b)

Sulfur, because it has 16 electrons

c)

Sodium, because it has 11 electrons

19.

What is the correct name for Cu(NO3)2?

a)

Copper (II) Nitrate

b)

Copper Nitrate

c)

Copper (III) Nitrate

20.

How many nuetrons are in the atom Ag-109?

a)

62

b)

109

c)

47

21.

How do you find the number of valence electrons?

a)

atomic number

b)

group number

c)

period number

22.

A substance that is tightly packed together is most likely in what state of matter?

a)

solid

b)

liquid

c)

gas

23.

What is the Molar Mass of KOH?

a)

40

b)

16

c)

1

d)

57

24.

What is the formula for diarsenic pentaoxide?

a)

As2O5

b)

AsO5

c)

As2O

25.

What is the name of CuCl3?

a)

Copper (III) Chloride

b)

Copper (II) Chloride

c)

Copper Chloride

26.

How many moles are in 19.82 g Mg?

a)

1.23 mol Mg

b)

481.70 mol Mg

c)

1.00 mol Mg

d)

0.82 mol Mg

27.

What is the percent composition by mass of sulfur (S) in the compound MgSO4?

a)

20.22%

b)

19.85%

c)

26.64%

d)

28.64%

28.

Determine the mass of 4.20 moles of C6H12

a)

354 g

b)

84 g

c)

337 g

d)

421 g

29.
What is the molar mass of PbSO4
a)
303.3 g/mol
b)
294.7g/mol
c)
163.8g/mol
d)
372g/mol
30.
What is the empirical formula for the following molecular formula: C6H14
a)
C6H14
b)
C3H7
c)
CH2
d)
CH3
31.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
32.

Approved eye protection devices (such as goggles) are worn in the laboratory

a)

to avoid eye strain.

b)

to improve your vision.

c)

only if you don’t have corrective glasses.

d)

any time chemicals, heat or glassware are used.

33.

You have been injured in the laboratory (cut, burn, etc.). First you should

a)

visit the school nurse after class.

b)

see a doctor after school.

c)

tell the science instructor at once.

d)

apply first aid yourself.

34.

In a laboratory, the following should not be worn.

a)

loose clothing.

b)

dangling jewelry.

c)

sandals.

d)

all of the above.

35.

Which of the following is not part of the atomic theory?

a)

All matter is composed of tiny, invisible, indivisible particles called atoms

b)

Atoms of different elements are different.

c)

Atoms have a neutral charge

d)

Atoms of the same element are the same.

e)

Atoms cannot be created or destroyed, just rearranged.

36.

What subatomic particle has a positive charge in the atom? Where is it located?

a)

Proton- nucleus

b)

Proton- outside nucleus

c)

Neutron- nucleus

d)

Neutron- outside nucleus

37.

What subatomic particle has a negative charge in the atom? Where is it located?

a)

Proton- nucleus

b)

Proton- outside nucleus

c)

Electron- nucleus

d)

Electron- outside nucleus

38.

What subatomic particle has a negative charge in the atom? Where is it located?

a)

Proton- nucleus

b)

Proton- outside nucleus

c)

Electron- nucleus

d)

Electron- outside nucleus

39.

What subatomic particle has a neutral charge in the atom? Where is it located?

a)

Proton- nucleus

b)

Proton- outside nucleus

c)

Neutron- nucleus

d)

Neutron- outside nucleus

40.

What is the atomic number?

a)

Number of protons

b)

Number of neutrons

c)

Number of protons + neutrons

41.

What is the mass number?

a)

Number of protons

b)

Number of neutrons

c)

Number of protons + neutrons

42.

What is an isotope?

a)

Same element with different number of protons

b)

Same element with different number of neutrons

c)

Same element with different number of electrons

d)

Different elements

43.

Describe a covalent bond.

a)

A bond where electrons are gained or lost

b)

A bond between two metals

c)

A bond where electrons are shared

44.

Describe an ionic bond.

a)

A bond where electrons are gained or lost

b)

A bond between two metals

c)

A bond where electrons are shared

45.

What is the octet rule?

a)

When an atom has 8 electrons in the outer valence shell

b)

When you have 8 arms

c)

When an atom has a total of 8 electrons

d)

When an atom has more than 8 total electrons

46.

What are models that show all bonding and non-bonding (lone pair) electrons of each atom within a molecule or atom?

a)

Bohr model

b)

Lewis dot

c)

Chemical formula

47.

What represents shared electrons between valence shells of atoms?

a)

Paired dots

b)

Paired stars

c)

Single dots

d)

Single stars

48.

CaF2

a)

Sodium hydrogen sulfate

b)

Copper (II) sulfite

c)

Potassium oxalate

d)

Calcium fluoride

49.

oxygen dichloride

a)

OF2

b)

PCl5

c)

OCl2

d)

BrCl5

50.

bromine pentachloride

a)

OF2

b)

PCl5

c)

OCl2

d)

BrCl5

51.

SCl6

a)

Diphosphorus pentoxide

b)

Sulfur hexachloride

c)

Carbon tetrachloride

d)

Silicon dioxide

52.

P2O5

a)

Diphosphorus pentoxide

b)

Sulfur hexachloride

c)

Carbon tetrachloride

d)

Silicon dioxide

53.

How many moles are there in 458 grams of Na2SO4?

a)

3.3 x 10-5 mol

b)

1257.11 g

c)

46.01 g

d)

3.22 mol

54.

How many grams are there in 7.40 moles of AgNO3?

a)

3.3 x 10-5 mol

b)

1257.11 g

c)

46.01 g

d)

3.22 mol

55.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
56.
Balance this equation
_Al +_HCl --> _H2 +_AlCl3
a)
2, 6, 3, 2
b)
it is already balanced
c)
4, 12, 3, 4
d)
2, 1, 4, 5
57.
Balance this equation.
_CH4 + _O2 --> _CO2 + _H2O
a)
1,2,1,1
b)
2,1,2,1
c)
1,2,1,2
d)
0,2,0,2
58.
25 mL of a mystery liquid has a mass of 37.5 grams. What is the density of the liquid?
a)
937.5 g/mL
b)
0.67 g/mL
c)
1.5 g/mL
d)
62.5 g/mL
59.
Which is a halogen?
a)
Fluorine
b)
Carbon
c)
Helium
d)
Lithium
60.
Which is a halogen?
a)
Fluorine
b)
Carbon
c)
Helium
d)
Lithium
61.
Which is an alkaline earth metal?
a)
Calcium
b)
Rubidium
c)
Carbon
d)
Iodine
62.
Which element is in group 4 period 6?
a)
Helium
b)
Chromium (Cr)
c)
Hafnium (Hf)
d)
Barium
63.
Sodium (Na)
a)
alkali metal
b)
alkaline earth metal
c)
halogen
d)
noble gas
64.
a)
Alkali
b)
Alkaline Earth
c)
Halogen
d)
Noble Gases
65.
a)

Transition Metals

b)

Inner Transition Metals

c)

Metals

d)

Metalloids

66.
What do atoms that form positive ions tend to do?
a)
Tend to lose electrons 
b)
Tend to lose protons
c)
Tend to gain electrons
d)
Tend to gain protons
67.
What usually forms the positive ion?
a)
Metal
b)
Non Metals
c)
None
68.
What usually forms the negative ion?
a)
nonmetals
b)
metal
c)
none
69.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
70.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
71.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
72.
Why is it called the Law of Conservation of Matter/Mass? 
a)
Energy is created and destroyed 
b)
Energy is never created, nor destroyed-- it always moves 
c)
Energy moves between particles
d)
Energy stops moving at the end of the universe 
73.
C-12 and C-14 are known as...
a)
Ions
b)
Isotopes
c)
Protons
d)
explosives 
74.
Which has the greater EN: 
N or C?
a)
C
b)
N
75.
Which has the greater EN: 
H or F?
a)
H
b)
F
76.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
77.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
78.
 Which of the following generally applies to the noble gases? 
a)
high ionization energy, low electronegativity, high reactivity
b)
high ionization energy, high electronegativity, high reactivity
c)
low ionization energy, low electronegativity, low reactivity
d)
high ionization energy, low electronegativity, low reactivity 
79.
What is ionization energy?
a)
Energy needed to destroy an atom
b)
Energy required to remove an electron
c)
Energy needed to split an electron
d)
Energy required to add an electron
80.

As you look down a group, ionization energy and electronegativity

a)

increases

b)

decreases

81.

As you look from left to right across a period, ionization energy and electronegativity both

a)

increase

b)

decrease

82.

Which element has the greater ionization energy?

a)

Magnesium (Mg)

b)

Phosphorus (P)

83.
List the following in order of weakest to strongest ionization energy.
P, Cs, Co, Sr
a)
P, Co, Sr, Cs
b)
Cs, Sr, Co, P
c)
Sr, Cs, Co, P
d)
P, Co, Cs, Sr

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