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Semester 1 Grand Summary

Total questions: 100

Worksheet time: 50mins

Name
Class
Date
1.

The kinetic theory states

a)

Particles won't move if you don't apply energy to it.

b)

Particles only move in liquids and gases.

c)

Particles are always in motion.

d)

At the same temperature the object that has the most mass heats quicker.

2.

The energy of movement is ___.

a)

potential energy

b)

kinetic energy

c)

mechanical energy

3.

The more energy that particles have, the ___ they move.

a)

slower

b)

faster

4.

The force of attraction between molecules is ___.

a)

intermolecular forces

b)

bridge forces

c)

chemical bonds

5.

These properties describe a ___.

a)

solid

b)

liquid

c)

gas

6.

These properties describe a ___.

a)

solid

b)

liquid

c)

gas

7.

These properties describe a ___.

a)

solid

b)

liquid

c)

gas

8.

Collisions in which particles transfer all their kinetic energy to other particles are called ___.

a)

elastic

b)

inelastic

9.

Which one of these is NOT an Ideal Gas Assumption?

a)

Gas particles are hard, round spheres.

b)

Gas particles are strongly attracted to one another.

c)

Gas particles do not take up space.

d)

Gas particles collide perfectly elastically.

10.

The particles of ___ generally have the least amount of energy.

a)

solids

b)

liquids

c)

gases

11.

Liquid particles have more energy than ___ particles.

a)

solid

b)

gas

12.

Diffusion occurs only in gases

a)

True

b)

False

13.

The movement of particles is __________, resulting in the particles being spread throughout the container

a)

Structured

b)

In a straight line

c)

Random

d)

In curved, way motions

14.

What does a 'region with high concentration' mean?

a)

SMALL number of particles

b)

LARGE number of particles

c)

UNEVEN number of particles

d)

no particles

15.

The picture below is an example of _________________.

a)

osmosis

b)

isotonic

c)

diffusion

d)

active transport

16.

Where is there a low concentration of dye?

a)

at the bottom of cup

b)

in the color

c)

at the top of cup

d)

no concenteraion gradient

17.
Which diagram best shows the end result of diffusion?
a)
F
b)
G
c)
H
d)
J
18.

What is DIFFUSION?

a)
b)
19.

Which BEST describes the meaning of mass of an object?

a)

The amount of space an object or substance takes up

b)

Mass divided by volume

c)

The amount of matter in an object or substance

d)

The weight of an object only in solid form and in zero gravity

20.

Which of the following BEST describes volume?

a)

How much space an object takes up

b)

Where an object is in space

c)

How much an object weighs

d)

The mass of an object compared to its weight

21.

What two properties do you need to find density?

a)

Volume and weight

b)

Mass and volume

c)

Only volume

d)

Only mass

22.

If an object sinks in water than it is (a)   than water and

23.

 If an object floats in water then it is (a)   than water.

24.

If I cut a block of gold in half, what happens to its density?

a)

Density is cut in half.

b)

Density stays the same.

c)

Density doubles.

d)

Density cannot be determined.

25.
Put the liquids in order from most dense to least dense?
a)
4, 3, 2, 1
b)
1, 2, 3, 4
c)
3, 4, 2, 1, 
d)
4, 3, 1, 2
26.
Which liquid is the least dense?
a)
oil
b)
water
c)
syrup 
d)
plastic bottle
27.
Look at this image.  Which object has the LOWEST density in water? How? 
a)
The Ping Pong Ball because it floats to the top 
b)
The bolt because it has sunk to the bottom
c)
The soda cap because it is not just full of air like the Ping Pong ball
28.

What is the most likely result of nitrogen and chlorine reacting based on their dot diagrams?

a)

Three chlorine atoms will each steal one electron from nitrogen

b)

Five chlorine atoms will each steal one electron from nitrogen

c)

Three chlorine atoms will each share one electron with nitrogen

d)

Five chlorine atoms will each share one electron from nitrogen

29.

Which of the following isotopes has 18 neutrons?

a)

40Ar

b)

35Cl

c)

18F

d)

24Mg

30.

As the number of protons increases across a period, while electrons are added to the same energy level, all of the following are true EXCEPT:

a)

the effective nuclear charge increases

b)

the electron shielding increases

c)

the atomic radius decreases

d)

the ionization energy increases

31.

Electronegativity _______ across a period and ______ down a group.

a)

increases, increases

b)

increases, decreases

c)

decreases, increases

d)

decreases, decreases

32.

Which of these atoms is the most electronegative?

a)

Bromine

b)

Fluorine

c)

Hydrogen

d)

Potassium

33.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

34.
Partial charges like the ones shown here are called:
a)
dipoles
b)
deltas
c)
ions
d)
magnetic poles
35.

The electrons in a nonpolar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

36.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

37.

CH4 is

a)

polar

b)

non-polar

38.

NH3 is

a)

polar

b)

non-polar

39.

Which of these atoms is the most electronegative?

a)

Bromine

b)

Fluorine

c)

Hydrogen

d)

Potassium

40.

Is the following molecule polar or non-polar?

a)

polar

b)

non-polar

41.

Electronegativity refers to an atom's ability to _____________ shared electrons in a covalent bond.

a)

attract

b)

donate

42.

H2O is

a)

polar 

b)

non-polar

43.

More electronegative atoms in covalent compounds are likely to have:

a)

Partial positive charge

b)

Partial negative charge

44.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

45.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar
46.

Why is the molecule polar?

a)

There is a non bonding pair electrons on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no non bonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

47.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

48.

Classify the above molecule.

a)

Polar

b)

Non polar

49.
What geometry will this molecular structure have?: PH3
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
50.

What is ionization energy?

a)

Energy needed to destroy an atom

b)

Energy required to remove an electron from an atom in its gaseous state

c)

Energy needed to split an electron

d)

Energy associated with how strongly an atom attracts electrons

51.

Electronegativity is...

a)

the measure of how strongly an atom attracts electrons

b)

the ability of an atom to lose electrons

c)

the energy required to remove an electron from a specific atom in its gaseous state

d)

how easy it is to make friends.

52.

What is the atomic radius?

a)

The distance from the nucleus to the outer boundary of an atom

b)

The distance from one side of an atom to the other side

c)

The distance around the atom

d)

The distance between atoms in the gas phase

e)

The distance between atoms in the solid phase

53.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
54.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
55.

As you move across the periodic table atoms tend to get smaller because, ______________.

a)

the atoms have more mass.

b)

the atoms have less mass

c)

the atoms have a bigger effective nuclear charge

d)

the atoms have less electrons.

56.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

57.

Which of these elements has the smallest atomic radius?

a)

C

b)

Ne

c)

K

d)

Al

e)

P

58.

Atomic radius generally increases as we move __________.

a)

down a group and from right to left across a period

b)

up a group and from left to right across a period

c)

down a group and from left to right across a period

d)

up a group and from right to left across a period

59.
How many neutrons would Fe-56 have?
a)
56
b)
26
c)
30
d)
33
60.
How many protons does P-30 have?
a)
30
b)
16
c)
12
d)
15
61.
What element has 42 protons?
a)
Ca
b)
Mo
c)
Zr
d)
Po
62.
If an atom of nickel has a charge of +3, how many electrons does the atom have?
a)
28
b)
25
c)
26
d)
31
63.

What is the number of proton of the molecule?

a)

80

b)

120

c)

200

64.

What is the number of proton of the molecule?

a)

80

b)

120

c)

200

65.

What is the number of electron of the molecule?

a)

80

b)

120

c)

200

66.

What is the number of neutron of the molecule?

a)

80

b)

120

c)

200

67.

What is the number of proton of the molecule?

a)

29

b)

34

c)

63

68.

How many atoms of hydrogen are in this compound?

a)

1

b)

2

c)

3

d)

4

69.

How many elements are in the compound Fe2O3?

a)

0

b)

1

c)

2

d)

3

70.

How many atoms of oxygen are in this compound?

2Ca(OH)2

a)

1

b)

2

c)

3

d)

4

71.

Find the molar mass of CaCO3CaCO_3   

a)

100.09g

b)

100g

c)

100.2g

d)

101g

72.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
73.

What is the mass of one mole of aluminum?

a)

27 g

b)

13 g

c)

54 g

d)

14 g

74.

What is the molar mass of NaOH?

a)

40 g/mol

b)

39 g/mol

c)

24 g/mol

d)

57 g/mol

75.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
76.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
77.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
78.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
79.

What is MOLECULAR GEOMETRY of this molecule?

a)

Bent

b)

Trigonal Pyramidal

c)

Tetrahedral

d)

Linear

80.

What is MOLECULAR GEOMETRY of this molecule?

a)

Bent

b)

Trigonal Pyramidal

c)

Tetrahedral

d)

Octahedral

81.
All elements in the same group have the same number of ___.
a)
protons
b)
neutrons
c)
atomic mass units
d)
valence electrons
82.
The majority of elements on the periodic table are
a)
man made.
b)
nonmetals.
c)
metals.
d)
gases.
83.
Chlorine (Cl) is part of the _ family.
a)
alkali metals
b)
alkaline earth metals
c)
halogens 
d)
noble gases
84.
Magnesium (Mg) is part of the _ family.
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
85.
Which group of elements have the most reactive nonmetals?
a)
metalloids
b)
halogens
c)
alkali metals
d)
noble gases
86.
Which group of elements have the most stable, nonreactive elements (will not bond with others)?
a)
metalloids
b)
halogens
c)
alkali metals
d)
noble gases
87.
How many valence electrons does an alkaline earth metal have? 
a)
1
b)
2
c)
7
d)
8
88.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
89.

Which type of elements form ionic compounds?

a)

metal + metal

b)

metal + nonmetal

c)

nonmetal + nonmetal

d)

metal + nonmetal + nonmetal

90.

Which type of elements form covalent compounds?

a)

metal + metal

b)

metal + nonmetal

c)

nonmetal + nonmetal

d)

metal + nonmetal + nonmetal

91.

Which type of compound is KBr, potassium bromide?

a)

covalent

b)

metallic

c)

ionic

d)

compound

92.

Which type of compound is N2O3N_2O_3 , dinitrogen trioxide?

a)

covalent

b)

metallic

c)

ionic

d)

compound

93.

What element is this?

a)

Boron

b)

Lithium

c)

Oxygen

d)

Sulfur

94.

How many energy levels does this atom have?

a)

1

b)

2

c)

3

d)

4

95.

How many energy levels does this element have?

a)

Unknown - it represents any element with seven valence electrons.

b)

1

c)

2

d)

3

96.

Draw the Bohr Diagram for B. How many valence electrons does B have?

a)

1

b)

2

c)

3

d)

4

97.
A covalent bond is
a)
a bond that shares electrons metallicaly
b)
A bond that shares electrons with non metals
c)
Metalloids bonding
d)
metals and nonmetals bonding
98.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
99.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
100.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D

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