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Physical Science Unit 4 Review

Total questions: 62

Worksheet time: 3hrs 38mins

Name
Class
Date
1.

How many VALENCE ELECTRONS does Chlorine have?

a)

2

b)

7

c)

8

d)

10

e)

17

2.

Ionic bonds are formed when electrons get

a)

Shared between two atoms

b)

Removed from both atoms

c)

Transferred from one atom to another

d)

Added to both atoms

3.

Ionic bonds typically form between

a)

A metal and a nonmetal

b)

Two nonmetals

c)

Two metals

d)

A metalloid and a metal

4.

What is the correct formula for Sodium Chloride?

a)

SCl

b)

NaCl

c)

SC

d)

NaCl2

5.

Name this ionic compound: Al2O3

a)

Dialuminum oxide

b)

Aluminum oxygen

c)

Oxygen Aluminide

d)

Aluminum oxide

6.

If you were to draw the lewis dot structure for Germanium (Ge), how many dots would you put around it?

a)

2

b)

4

c)

6

d)

8

7.

Cations _______ electrons, becoming _______ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

8.

Anions ____ electrons, becoming _____ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

9.

Write the chemical formula for K and Br (potassium bromide).

a)

KBr

b)

K2Br

c)

KBr3

d)

KBr2

10.

Write the chemical formula for Na and S (sodium sulfide).

a)

NaS

b)

S2S2

c)

Na2S

d)

NaS2

11.

Lead Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

12.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

13.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

14.

Generally low melting and boiling points

a)

Ionic compounds

b)

Covalent compounds

15.

Generally high melting & boiling points

a)

Ionic compounds

b)

Covalent compounds

16.

Can be a solid, liquid, or gas at room temperature

a)

Ionic compounds

b)

Covalent compounds

17.

Poor electrical conductivity

a)

Ionic compounds

b)

Covalent compounds

18.

Valence electrons are shared

a)

Ionic bonds

b)

Covalent bonds

19.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
20.

The chemical bond between a non-metal and another non-metal will be a ________ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

21.

The chemical bond between a metal and a non-metal will be a _____ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

22.

Sodium and Bromine will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

23.

Carbon and Oxygen will make a ___________ bond.

a)

ionic

b)

covalent

c)

metallic

24.

MgO

a)

ionic

b)

covalent

c)

metallic

25.

If two fluorine atoms bond they will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

26.
Ionic bonds form between two ions that have...
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
27.
Which is most likely to form a negative ion...
a)

an element from Group 7

b)
a metal
c)
an element from Group 1
d)
an element with atoms that have eight valence electrons
28.
A(n) _____________ is an atom or group of atoms that has an electric charge. 
a)
ion
b)
electron
29.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
30.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
31.

dinitrogen pentoxide

a)

N2O5

b)

NO5

c)

N5O2

d)

N2O6

32.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
33.

P₄S₁₀

a)

tetrapotassium decasulfide

b)

phosphorus decasulfide

c)

tetraphosphorus decasulfide

d)

phosphorus (X) sulfide

34.

SO₃

a)

sulfate

b)

sulfur oxide

c)

sulfur trioxide

d)

monosulfur trioxide

35.

What is the OFFICIAL name for H2O? Hint.. This is a trick question so choose carefully!

a)

Hydrogen Oxide

b)

Oxygen Dinitride

c)

Water

d)

Dihydrogen Monoxide

36.

LiBr is called

a)

lithium bromine

b)

lithium monobromine

c)

lithium bromide

d)

lithuim monobromide

37.

Which is the correct formula for the compound: Calcium Oxide

a)

CaO

b)

CaO2

c)

Ca2O

38.
What is the correct formula for Sodium Oxide?
a)
NaO
b)
NaO2
c)
Na2O
d)
Na2O2
39.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
40.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
41.

If an element is diatomic it should have a subscript of___

a)

1, always

b)

2, only when it is an element

c)

it shouldn't have a subscript, it should have a coefficent

d)

2, when bonded in a compound

42.

Predict the products of this synthesis reaction: H2 + Cl2 →

a)

HCl

b)

H2Cl2

c)

H2Cl

d)

HCl2

43.

Predict the products for the this Single Replacement reaction:

K + HCl →

a)

KCl + H2

b)

KHCl

c)

KH + Cl2

d)

HCl + K2

44.

Predict the products for the this Single Replacement reaction: (Copper has a charge of 1+)

Mg + CuCl →

a)

MgCl2 + Cu

b)

Mg + Cu

c)

MgCu + Cl2

d)

MgCl + Cu2

45.

Predict the product of this synthesis reaction:

Al + S₈ →

a)

AlS

b)

AlS8

c)

Al2S

d)

Al2S3

46.

Predict the products for the decomposition of aluminum oxide, Al2O3 →

a)

Al + O2

b)

O + Al2

c)

Al2 + O3

d)

Al + O

47.

Based on the information provided what type of reaction it this?


Au2S3 + 3 H2 ➔ 2 Au + ____________

a)

Combustion

b)

Single replacement

c)

Double replacement

d)

Synthesis

48.

What would the missing product be?


Au2S3 + 3 H2 ➔ 2 Au + ____________

a)

2 H3S

b)

2 AuH3

c)

3 H2S

49.

Based on the information provided, what type of reaction is this?


Fe + O2 ➔ ___________

a)

Double replacement

b)

Single replacement

c)

Synthesis

d)

Decomposition

50.

What would the missing product be?


Fe + O2 ➔ ___________

a)

Fe2O2

b)

2 FeO

c)

2 FeOH

51.

Based on the information provided, what type of reaction is this?


2 NO2 ➔ O2 + _________

a)

Double replacement

b)

Single replacement

c)

Synthesis

d)

Decomposition

52.

What is the missing product?


2 NO2 ➔ O2 + _________

a)

N2

b)

N

c)

NO

53.

…NaCl + …F2 → …NaF +…Cl2\ldots NaCl\ +\ \ldots F_2\ \rightarrow\ \ldots NaF\ +\ldots Cl_2  balance the equation

(a)  

54.

…H2 +…O2 → …H2O\ldots H_2\ +\ldots O_2\ \rightarrow\ \ldots H_2O  balance the equation

(a)  

55.

…P + …O2 → …P2O5\ldots P\ +\ \ldots O_2\ \rightarrow\ \ldots P_2O_5   balance the equation

(a)  

56.

…S8 + …O2 → …SO3\ldots S_8\ +\ \ldots O_2\ \rightarrow\ \ldots SO_3  balance the equation

(a)  

57.

Is the following reaction endothermic or exothermic

a)

endothermic

b)

exothermic

58.

Is the following reaction endothermic or exothermic

a)

endothermic

b)

exothermic

59.

If the size of an object decreases, surface area ________.

a)

decreases

b)

increases

60.

Indicate whether each of the following will: Increase / Decrease / have No effect on the rate of reaction.

 

                Increasing temperature

              

a)

Increase

b)

Decrease

c)

No Effect

61.

Indicate whether each of the following will: Increase / Decrease / have No effect on the rate of reaction.

 

                Decrease Reactant Concentration             

a)

Increase

b)

Decrease

c)

No Effect

62.

When surface area increases, the reaction rate

a)

decreases

b)

increases

c)

does not change

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