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Interim Assessment Review

Total questions: 62

Worksheet time: 47mins

Name
Class
Date
1.
Determine the type of bond in an oxygen molecule (O2). HINT: Use (IE - AE)/2 = # of bonds.
a)
Double covalent
b)
Single covalent
c)
Ionic
d)
Triple covalent
2.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
3.
If electrons are shared unequally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
4.
How strongly an atom attracts electrons is called....................
a)
Ionization energy
b)
Electronegativity
c)
Electricity
d)
Nuclear force
5.

What determines where the habitable zone is located for each star?

a)

The star's distance from Earth

b)

The size of the star

c)

How many planets the star has

d)

The size of the planet

6.
In order for life as we know it to exist, a planet must have ______________________
a)
heat
b)
animals
c)
liquid water
d)
solar energy
7.
An exoplanet is:
a)
a planet that is about to supernova.
b)
any planet outside of our Solar System.
c)
too small to be a regular planet - like Pluto :(
d)
usually very similar to Earth.
8.

What is a positive ion called?

a)

anion

b)

cation

c)

isotope

d)

covalent

9.

What is a negative ion called?

a)

anion

b)

cation

c)

covalent

d)

isotope

10.

Which types of elements from cations?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

11.

Which types of elements from anions?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

12.

Why do elements form bonds?

a)

to get a charge

b)

so they can make friends

c)

to become stable by getting a full valence shell

d)

to become stable by increasing their mass

13.

How many electrons would a Nitrogen ion gain/lose?

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

14.

How many electrons would a Calcium ion gain/lose?

a)

lose 1

b)

gain 1

c)

lose 2

d)

gain 2

15.

What is the ion formed from Sulfur?

a)

S+2

b)

S-2

c)

S+6

d)

S-6

16.

If an atom loses electrons, the charge will be positive.

a)

true

b)

false

17.

Be ionizes to a charge of ________.

a)

+1

b)

+2

c)

-1

d)

-2

18.
Which of the following has a -3 charge?
a)
Boron
b)
Fluorine
c)
Nitrogen
d)
Neon
19.

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

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

20.

The electrons in an ionic molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

21.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

22.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

23.

Molecules that contain whole number charges on atoms (+1,-3, etc.) must be...

a)

Polar Covalent

b)

Nonpolar Covalent

c)

Ionic

d)

Polar Covalent or Ionic

24.

In a polar covalent bond, which atom will have a partial positive charge? (choose 2 correct answers)

a)

The atom that attracts fewer electrons

b)

The atom with the greater electronegitivity

c)

The atom that attracts more electrons

d)

The atom with the lower electronegativity

25.

What must the difference in electronegativity between two atoms be in order for the bond between them to be polar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

26.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

27.

Order the types of bonds based on the charge of their molecules. (lowest amount of charge to greatest)

a)

Polar Covalent --> Ionic --> Nonpolar Covalent

b)

Ionic --> Nonpolar Covalent --> Polar Covalent

c)

Ionic --> Polar Covalent --> Nonpolar Covalent

d)

Nonpolar Covalent --> Polar Covalent --> Ionic

28.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

29.

When you have Be-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

30.

How would the melting point and boiling point for polar covalent bond?

a)

High

b)

Low

31.

How would the melting point and boiling point for nonpolar covalent bond?

a)

High

b)

Low

32.

What would solubility look like for polar covalent bond in water?

a)

soluable

b)

nonsoluable

33.

What would solubility look like for nonpolar covalent bond in water?

a)

soluable

b)

nonsoluable

34.
Which of the following is a polar molecule?
a)
CH4
b)
Xe
c)
H2O
d)
CO2
35.
Which statement correctly describes NaCl?
a)
Its charge is evenly distributed
b)
It is a polar molecule
c)
It is ionic, and its charges are distributed unevenly
36.
Which of the following molecules, based on the elements present, would be most polar?
a)
HF
b)
H2
c)
HCl
d)
HBr
37.
Which statement explains why ethene does not dissolve in water?
a)
Ethene is polar and water is nonpolar.
b)
Ethene is nonpolar and water is nonpolar.
c)
Ethene is polar and water is polar.
d)
Ethene is nonpolar and water is polar.
38.

Mg and Cl create...

a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
39.

H and S create...

a)
H2S
b)
HS2
c)
H2S2
d)
HS
40.

Ca and N create...

a)
Ca2N3
b)
Ca3N2
c)
CaN3
d)
Ca2N
41.

Al and P create...

a)

Al3P

b)

AlP3

c)

AlP

d)

Al2P

42.
Carbon is considered an element while carbon dioxide is considered a compound. This is because carbon dioxide is –
a)
a gas at room temperature.
b)
made of two different elements.
c)
given off by green plants.
43.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
44.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
45.
What is the name of a single type of atom?
a)
cell
b)
proton
c)
element
d)
atom
46.

Which of the following substances would conduct electricity if dissolved in water to form a solution?

a)

C6H12O6

b)

CH4

c)

KI

d)

CO2

47.

A conductivity tester is placed in a solution of water and an unknown solute. The bulb doesn't light up. What can you determine about the unknown solute?

a)

It is an ionic compound.

b)

It is a metallic compound.

c)

It is a covalent compound.

d)

Not enough information is given to answer this question.

48.

A light bulb connected to two electrodes is immersed in the following solutions. Which one will make the light bulb light up the brightest?

a)

1 g of sugar in 1 cup of water

b)

1 g of salt in 1 cup of water

c)

10 g of salt in 1 cup of water

d)

10 g of sugar in 1 cup of water.

49.

Which of the following will produce ions to conduct electricity when dissolved in water?

a)

CaCl2

b)

NH3

c)

CH4

d)

P2O5

50.

Which diagram best illustrates the ion-molecule attractions that occur when the ions of NaCl(s) are added to water?

a)

1

b)

2

c)

3

d)

4

51.

A solid substance was tested in the laboratory. The test results are listed below.

• dissolves in water

• is an electrolyte

• melts at a high temperature

Based on these results, the solid substance could be

a)

Cu

b)

CuBr2

c)

C

d)

C6H12O6

52.

A substance that conducts an electrical current when dissolved in water is called

a)

catalyst

b)

metalloid

c)

electrolyte

d)

nonelectrolyte

53.

What type of electromagnetic wave has a higher frequency than visible light and a larger wavelength than x-rays

a)

Infrared

b)

Gamma

c)

visible

d)

Ultraviolet

54.

Indicate the electromagnetic waves that are longer than Visible light.

a)

Ultraviolet

b)

Infrared

c)

X ray

d)

Microwaves

55.

What type of wave has the largest wavelength and the lowest frequency on the electromagnetic spectrum?

a)

Radio

b)

Micro

c)

Gamma

d)

X ray

56.

Which electromagnetic waves are useful for Television?

a)

Gamma

b)

x ray

c)

radio

d)

microwave

57.

The medical profession uses _______ to sterilize medical equipment - just like the google cabinet in the science classroom.

a)

Infrared

b)

x ray

c)

Gamma

d)

Ultraviolet

58.

Each element on the periodic table can be identified by its

a)

classification as a solid, liquid or gas.

b)

location on the table.

c)

ability to react to form compounds.

d)

unique spectral "fingerprint."

59.

What subatomic particle is responsible for the spectral lines seen in emission spectra diagrams?

a)

electrons

b)

protons

c)

neutrons

60.

In order to go from ground state to an excited state, an electron must

a)

emit energy

b)

absorb energy

c)

wiggle

61.

When an electron returns to ground state from an excited state, the atom will

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

62.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D

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