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ICP Unit 4 Review

Total questions: 50

Worksheet time: 37mins

Name
Class
Date
1.
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
2.
What usually forms the positive ion?
a)
Metal
b)
Non Metals
c)
None
3.
What usually forms the negative ion?
a)
nonmetals
b)
metal
c)
none
4.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
5.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
6.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
7.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
8.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
9.
What is a valence electron?
a)
an electron that is found in the outermost shell of an atom. 
b)
an electron found in the innermost shell of an atom.
c)
an electron found in the middle shell.
10.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
11.
What is the number of valence electrons for Beryillum?
a)
1
b)
4
c)
2
d)
7
12.
What is the number of valence electrons for Neon?
a)
6
b)
7
c)
8
d)
9
13.
A chemical bond resulting from the electrostatic attraction between positive and negative ions is called a(n)
a)
covalent bond.
b)
ionic bond.
c)
charged bond.
d)
dipole bond.
14.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
15.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
16.
The force that hold two atoms together is called a ______. 
a)
Chemical Change
b)
Reaction
c)
Chemical Bond
d)
Physical Change
17.
How many electrons does chlorine need to gain in order to have a full outer shell? 
a)
7
b)
0
c)
1
d)
8
18.
A charged Particle is called an 
a)
isotope
b)
Ion
c)
Molecule
d)
Compound
19.
The number of _____ is most important in determining how an atoms will bond. 
a)
Neutrons
b)
Protons
c)
Valence Electrons
d)
Electron sin the innermost shell
20.
How does a selenium atom attain a noble gas electron configuration?
a)
it loses two electrons
b)
it gains two electrons
c)
it loses six electrons
d)
it gains six electrons
21.
Which of the following best describes a metallic bond?
a)
Metal cations are attracted to metal anions
b)
Metal atoms share pairs of valence electrons equally
c)
Metal atoms share pairs of valence electrons unequally
d)
Metal share a "sea" of valence electrons
22.
Two atoms of chlorine bond to form a diatomic molecule. Which type of bond exists between the two atoms?
a)
a Nonpolar covalent bond
b)
Polar covalent bond
c)
ionic bond
d)
hydrogen bond
23.
What type of substance has a very low melting point, is insoluble in water and does not conduct electricity?
a)
a Nonpolar molecular substance
b)
a polar molecular substance
c)
an ionic substance
d)
a metallic substance
24.

dinitrogen tetraoxide

a)

N4O2

b)

N2O4

c)

N2O5

d)

N4O

25.
What is the proper name for Cu2O?
a)
Copper oxide
b)
dicopper oxide
c)
copper (II) oxide
d)
copper (I) oxide
26.
barium hydroxide
a)
Ba(OH)2
b)
Ba2OH
c)
BaOH
d)
Ba2OH
27.
Ca+2 combines with Br- to form
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
28.
Name that Compound:
MgF2
a)
magnesium fluoride
b)
manganese Phosphide
c)
magnesium(III) fluoride
d)
magnesium fluoride(II)
29.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
30.
What is the name of the covalent molecule C4H10?
a)
Tetracarbon Decahydroxide
b)
Tetracarbon Decahydride
c)
Carbon Hydroxide
d)
Tetracarbon Decahydrogen
31.

Which of the following is NOT covalently bonded?

a)

K2S

b)

H2O

c)

I2

d)

CO2

32.
What is the formula for chromium (I) selenide?
a)
Cr2Se
b)
CrSe
c)
CrSe2
d)
Cr2Se2
33.
What is a cation?
a)
positive ion
b)
Neutral atom
c)
Two additional protons
d)
negative ion
34.
What is an anion?
a)
positive ion
b)
negative ion
c)
neutral atom
d)
2 neutrons taken away
35.
Most elements will gain or lose electrons so that they end up with _______ valence electrons.
a)
2
b)
6
c)
8
d)
10
36.
What element in period 2 has 7 valence electrons?
a)
Beryllium
b)
Chlorine
c)
Magnesium
d)
Fluorine
37.
Which element has the same number of electrons in the outermost energy level as lithium?
a)
Hydrogen
b)
Beryllium
c)
Carbon
d)
Magnesium
38.

What is a molecule?

a)

two elements bonded together (sharing electrons)

b)

a mixture of different substances

c)

smallest individual particles

d)

two elements bonded together (transferring electrons)

39.
How many total atoms are in the compound C2H8O ?
a)
11
b)
2
c)
8
d)
1
40.
Energy that is stored in bonds between atoms is:
a)
Mechanical energy
b)
Chemical energy
c)
Kinetic energy
d)
Nuclear energy
41.
What group of elements satisfies the octet rule without forming compounds?
a)
halogen
b)
noble gas
c)
alkali metal
d)
alkaline-earth metal
42.

Alkaline earth metals form ions with _____ charge

a)

-1

b)

+1

c)

+2

d)

-2

43.

The small numbers written below the symbol that tells you how many atoms there are.

a)

chemical symbol

b)

chemical formula

c)

subscript

d)

coefficient

44.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

45.

What type of chemical bond is represented in this diagram?

a)

double covalent bond

b)

single covalent bond

c)

ionic bond

d)

metallic bond

46.
2. Which of the following elements are not found as diatomic molecules?
a)
a) Hydrogen
b)
b) Chlorine
c)
c) Helium
d)
d) Nitrogen
47.
11. Which of the following physical properties is not typical of metals?
a)
a) Sonorous
b)
b) Electrical Conductor
c)
c) Low melting point
d)
d) Maleable
48.

An alloy is a mixture of a(n) ____ and one or more other elements.

a)

metal

b)

organic compound

c)

ceramic

d)

plastic

49.

How does increasing the amount of carbon in steel affect its properties?

a)

Carbon makes the lattice harder and stronger.

b)

Carbon forms an oxide that protects the steel from rusting.

c)

Carbon makes the steel light enough to use for airplane parts.

d)

Carbon makes the steel softer and easier to cut.

50.

What does the element symbol in an electron dot diagram represent?

a)

the nucleus of the atom.

b)

the nucleus and all electrons.

c)

the nucleus and valence electrons.

d)

the nucleus and all non-valence electrons.

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