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Unit 5/5b Review

Total questions: 47

Worksheet time: 52mins

Name
Class
Date
1.

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

a)

Metal

b)

Covalent

c)

Ionic

2.

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

a)

Metal

b)

Ionic

c)

Covalent

3.

Beryllium and sulfur will form a ______ bond

a)

Ionic

b)

Covalent

c)

Metalloid

4.

Sodium and Bromine will make a _____ bond.

a)

Ionic

b)

Covalent

c)

Metallic

5.

Carbon and Oxygen will make a ___________ bond.

a)

Ionic

b)

Covalent

c)

Metallic

6.

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

a)

Ionic

b)

Covalent

c)

Metallic

7.

Ionic compounds are formed when one or more valence electrons are transferred from _____

a)

a nonmetal atom to a metal atom

b)

a metal atom to a nonmetal atom

c)

a nonmetal atom to a nonmetal atom

d)

a metal atom to a metal atom

8.

What kind of bond(s) are shown?

a)

Ionic

b)

Covalent

c)

Metallic

9.

How many shared pairs of electrons are shown?

a)

1

b)

2

c)

4

d)

5

10.

True or false: An atom becomes a positive ion when it gains an electron.

a)

True

b)

False. It becomes a neutral ion!

c)

False. It becomes a negative ion!

11.

Table Salt (NaCl) creates crystals. What type of bond is present in this compound?

a)

Covalent

b)

Ionic

c)

Moleculuar

d)

Metallic

12.

What do the lines in this water molecule represent?

a)

A chemical bond

b)

Sharing of electrons

c)

A mixture

13.

Which type of bonds will conduct electricity?

a)

Ionic

b)

Covalent

c)

Molecular

d)

Metallic

14.

Chlorine gains 1 electron to complete the outermost energy level. What is it's charge?

a)

1+

b)

2+

c)

-1

d)

-2

15.

If an aluminum atoms loses its three valence electrons, its charge becomes____________________.

a)

3+

b)

0

c)

-3

d)

8

16.

Why do atoms bond?

a)

They typically don't bond

b)

To add or take away energy levels

c)

To have a full inner shell

d)

To have a full valence shell.

17.

What is the number of valence electrons for Carbon (Group 14)?

a)

1

b)

2

c)

4

d)

5

18.

Which sub-atomic particle is involved in chemical bonding?

a)

Protons

b)

Electrons

c)

Neutrons

d)

Valence electrons

19.

What is the valence / oxidation number for barium (Ba)?

a)

+1

b)

-1

c)

+2

d)

-2

20.

What is the correct formula for the compound, lithium oxide?

a)

LiO

b)

LiO2

c)

Li2O

d)

Li2O2

21.

Name the following ionic compound: MgSO4

a)

magnesium sulfoxide

b)

magnesium sulfate

c)

magnesium sulfide

d)

magnesium oxide

22.

The chemical compound for sodium phosphate would be:

a)

Na3PO4

b)

NaPO4

c)

Na2PO4

d)

Na(PO4)3

23.

When bonded together, the chemical formula for Mg2+ and Cl- will be...

a)

Mg2Cl

b)

Mg2Cl2

c)

MgCl2

d)

MgCl

24.

When bonded together, the chemical formula for Li+1 and P3- will be...

a)

Li3P

b)

LiP

c)

LiP3

d)

Li2P

25.

What does the Law of Conservation of Mass state?

a)

Matter cannot be gained or lost in a chemical reaction.

b)

Matter can only be gained in a chemical reaction.

c)

Matter can only be lost in a chemical reaction.

d)

Matter can be gained and lost in a chemical reaction. 

26.

What is the left part of a chemical equation called? 2H2 + O2 --> 2H2O

a)

Reactants

b)

Products

c)

Yield

27.

What is the right part of a chemical equation called...

2H2 + O2 --> 2H2O

a)

Reactants

b)

Products

c)

Yield arrow

28.

What is the number before a chemical formula called?

Ex: 2H2 + O2 --> 2H2O

a)

Coefficient

b)

Atom

c)

Subscript

d)

Equation

29.

Is the following chemical equation balanced?

Al + O2 --> 2Al2O3

a)

Yes

b)

No

30.

How many different elements are in C6H12O6?

a)

1

b)

2

c)

3

d)

4

31.

How many oxygen atoms are in Al2(SO4)3?

a)

4

b)

10

c)

8

d)

12

32.

Which of the following is the correct name for the chemical formula Li2S?

a)

Lithium sulfate

b)

lithium sulfite

c)

lithium sulfide

d)

lithium hyposulfite

33.

What is the formula for Sodium Oxide?

a)

NaO

b)

Na2O

c)

ONa

d)

NaO2

34.

What coefficient should be used to make the following equation balanced?

N2+O2--> _NO 

a)

1

b)

3

c)

2

d)

4

35.

How many HCl molecules do you need to balance this equation?

 Mg +  __HCl --->  MgCl2 + H2

a)

1

b)

3

c)

2

d)

4

36.

Identify the product(s) in the following chemical reaction:

Chromium oxide + Carbon → Chromium + Carbon monoxide

a)

Chromium and carbon.

b)

Chromium and carbon dioxide.

c)

Chromium oxide and carbon

d)

Chromium and carbon monoxide

37.

According to The Law of Conservation of Mass, how does the total mass of the products compare to the total mass of the reactants?

a)

They must be equal

b)

The mass of the reactants must be greater than the mass of the products

c)

The mass of the products must be greater than the mass of the reactants

38.

What do exothermic reactions do?

a)

Absorb energy

b)

Release color

c)

Release energy

d)

Absorb color

39.

A substance that increases speed of chemical reaction without being being changed is called:

a)

Catalyst

b)

Acid

c)

Base

d)

Pressure

40.

Grinding a tablet into powder increases the rate of reaction due to increased...

a)

Concentration

b)

Temperature

c)

Surface area

d)

Reactant

41.

If a chemical reaction is exothermic, the temperature would....

a)

Stay the same

b)

Decrease

c)

Increase

42.

Increasing the temperature of the reactants can do which of the following?

a)

Slow number of collisions thus increasing reaction rate

b)

Cause particles to lose speed thus decreasing reaction rate

c)

Increase collisions between the particles thus increasing the rate

43.

What do endothermic reactions do?

a)

Absorb heat energy, making the surroundings cooler

b)

Absorb heat energy, making the surroundings warmer

c)

Release heat energy, making the surroundings cooler

d)

Release heat energy, making the surroundings warmer

44.

Which of the following would INCREASE reaction rate?

a)

the particle size of the reactants is larger

b)

concentration of the reactants is increased

c)

temperature is decreased

d)

the reaction is not stirred

45.

Is this reaction exothermic or endothermic? Why?

a)

Exothermic, because it's creating/releasing heat energy

b)

Endothermic, because it's creating/releasing heat energy

c)

Exothermic, because it's absorbing heat energy

d)

Endothermic, because it's absorbing heat energy

46.

What type of chemical reaction is shown below?

K2S + MgCl2 −−> 2KCl +MgSK_2S\ +\ MgCl_2\ -->\ 2KCl\ +MgS

a)

Single replacement

b)

Double replacement

c)

Synthesis

d)

Decomposition

47.

What type of chemical reaction is shown below?

2Fe + 3Cl2 −−−> 2FeCl32Fe\ +\ 3Cl_2\ --->\ 2FeCl_3

a)

Single replacement

b)

Double replacement

c)

Synthesis

d)

Decomposition

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