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PShipman Carnegie PS SpS123 Georgia Review

Total questions: 32

Worksheet time: 16mins

Name
Class
Date
1.
Two atoms of different elements will definitely have different numbers_____
a)
Nuclei
b)
Protons
c)
Neutrons
d)
Electrons
2.
An ion forms when an atom gains or loses
a)
Protons
b)
Neutrons
c)
Electrons
d)

Mass

3.
A neutral atom would become an ion that has a charge of 2+ by 
a)
Losing two protons
b)
Losing two neutrons
c)
Losing two electrons
d)

Shared electrons

4.
Isotopes are atoms that have different
a)
Mass numbers
b)
Element names
c)
Atomic Numbers
d)

Locations on the PToE

5.
A positively charged ion is formed when
a)
A neutron is lost
b)
An electron is lost
c)
A neutron is gained
d)
An electron is gained
6.
Which of the following particle pairs has approximately the same mass?
a)
protons and neutrons
b)
protons and electrons
c)
neutrons and electrons
d)
protons, neutrons and electrons
7.
Iron-60 (atomic number 26) is an isotope that is often used to study meteorites.  How many neutrons does iron-60 have?
a)
26
b)
60
c)
34
d)
86
8.

Which of these molecules have the same number of Carbon Atoms?

a)

Substance 1 and 4

b)

Substance 2

c)

Substance 1 and 3

d)

Substance 2 and 4

9.

In what section would you most likely find an element that is a brittle solid at room temperature and is not a good conductor?

a)

Section 1

b)

Section 2

c)

Section 3

d)

There are no elements that are brittle solids

10.

What element has 6 Valence Electrons but only two (2) Energy shells/Orbitals?

a)

Gold

b)

Oxygen

c)

Barium

d)

Sulfur

11.

The following two elements:

a)

Have similar chemical properties and can be found in Group 7 of the periodic table

b)

Do not have similar chemical properties and are not in the same group

c)

Have similar chemical properties and can be found on opposite sides of the periodic table

d)

Have similar chemical properties and can be found in Group 2 of the periodic table

12.

Valence Electrons determine an element's___________________________, While Protons determine an element's____________________________.

a)

IDENTITY; REACTIVITY

b)

Both determine reactivity

c)

REACTIVITY; IDENTITY

d)

Both determine identity

13.

A researcher began the following reaction with 52.6 grams of sugar and Sulfiric Acid in part A. The final mass of the products in part B would MOST LIKELY be:

a)

More than 52.6 grams

b)

Less than 52.6 grams

c)

Exactly 52.6 grams

d)

Cannot be determined

14.

Which atom diagram has chemical properties most similar to carbon?

a)
b)
c)
d)
15.

The nucleus of the atom contains 8 protons and 9 neutrons. The atom is electrically neutral. How many electrons does this atom have?

a)

1

b)

8

c)

9

d)

15

16.
Which of the following is NOT formed by a covalent bond?
a)
K2S
b)
H2O
c)
I2
d)
CO2
17.
Which of the following is NOT considered a diatomic element?
a)
Carbon
b)
Nitrogen
c)
Chlorine
d)
Iodine
18.

How do the boiling points of ionic and covalent compounds compare?

a)

Boiling points for ionic compounds are lower than boiling points for covalent compounds.

b)

Boiling points for ionic compounds are higher than boiling points for covalent compounds.

c)

Boiling points for ionic compounds are approximately the same as boiling points for covalent compounds.

d)

Boiling points for ionic compounds are higher than boiling points for some covalent compounds and lower for other covalent compounds.

19.

Which of Deanna’s models correctly represents a stable calcium fluoride compound?

a)

b)

c)

d)

20.

How should you change the image below to represent an ionic bond between sodium and fluorine?

a)

move 7 electron from fluorine to sodium

b)

move one electron from fluorine to sodium

c)

move one electron from sodium to fluorine

d)

Nothing. The image already shows an ionic bond.

21.

Use IUPAC nomenclature rules to properly identify this compound: K2O

a)

potassium oxide

b)

dipotassium oxide

c)

potassium (I) oxide

d)

dipdipotassium monoxide

22.

Carbon Tetrafluoride

a)

C4F

b)

CF

c)

C4F4

d)

CF4

23.

Name this compound according to IUPAC nomenclature rules: NO

a)

nitrogen oxide

b)

nitrogen oxygen

c)

nitrogen monoxide

d)

mononitrogen monoxide

24.

What is the correct chemical formula for dinitrogen tetroxide?

a)

N2O4

b)

N2O3

c)

N3O2

d)

N4O2

25.

Which of the following formula and chemical name combinations is correctly shown?

a)

N2O2; nitrogen dioxide

b)

N2O5; dinitrogen pentoxide

c)

Ca2P3; dicalcium diphosphide

d)

PCl5; phosphorus tetrachloride

26.
10 g of a solid chemical reacts with a 10 g of a liquid chemical, the reaction bubbles and changes the color of the liquid.  The colored liquid weighs 13 g, what can be concluded?
a)
The gas produced from the bubbles weighed 5 g
b)
The bubbles were evidence of 7 g of matter being destroyed
c)
The gas produced weighed 7 g
d)
The gas produced weighed 13 g
27.

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

Mg + __HCl → MgCl2 + H2

a)

1

b)

2

c)

3

d)

4

28.

According to the Law of Conservation of Mass, how much zinc was present in the zinc carbonate?

a)

a. 25 grams

b)

b. 45 grams

c)

c. 65 grams

d)

d. 85 grams

29.

Which of the following best illustrates the Law of Conservation of Mass?

a)

a. H2SO4 → H2O + SO2

b)

b. H2SO4 → 2H2O2 + SO2

c)

c. 2H2SO4 → 2H2O + SO3

d)

d. H2SO4 → H2O + SO3

30.
What is the type of reaction shown at the top?
a)
Combination
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
31.
The following reaction is an example of what reaction type? 
CoCO3 → CoO + CO2
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
32.
Combining substances to form a new substance
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation

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