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Exam 1 Review - CP100

Total questions: 57

Worksheet time: 55mins

Name
Class
Date
1.

All matter is made of what...

a)

energy

b)

atoms

c)

electrons

d)

compounds

2.

The positive particles of an atom are

a)

electrons

b)

positrons

c)

neutrons

d)

protons

3.

The central region of an atom where its neutrons and protons are is its

a)

nucleus

b)

electron cloud

c)

core

d)

center

4.

Particles in an atom that are neutral and have no charge are

a)

negatrons

b)

electrons

c)

neutrons

d)

protons

5.
A particle that moves around the nucleus is a(n)...
a)
Proton
b)
Neutron
c)
Electron
d)
Quark
6.

What does the 1.00794 stand for?

a)

Hydrogen

b)

atomic number

c)

atomic mass

d)

atomic explosion

7.

In the modern periodic table, elements are arranged by:

a)

atomic mass

b)

atomic number

c)

valence electrons

d)

number of isotopes

8.

An atom with atomic number 6 would have how many protons

a)

6

b)

12

c)

3

d)

cannot be determined

9.

What is the number of protons that the element in this image contain?

a)

14

b)

7

c)

15

d)

18

10.
What are the 3 particles that make-up the atom?
a)
protons, neutrons, and isotopes
b)
neutrons, isotopes, and electrons
c)
positives, negatives, and electrons
d)
protons, neutrons, and electrons
11.

Why is the overall charge of an atom neutral (0)?

a)

They have the same number of protons and neutrons.

b)

They have the same number of protons and electrons.

c)

They have the same number of electrons and neutrons.

12.
How does the size of a proton compare to the size of a neutron?
a)
larger
b)
smaller
c)
equal
13.
These determine the reactivity of an element...
a)
Valence electrons
b)
Valence Protons
c)
Valence Neutrons
d)
Valence Quark
14.
Lithium is located in Group 1 of the Periodic Table, which element has similar characteristics of Lithium?
a)
Cesium (Cs)
b)
Beryllium (Be)
c)
Neon (Ne)
d)
Magnesium (Mg)
15.
Arsenic is located in Group 15 of the Periodic Table.  How many valence electrons does the arsenic atom have?
a)
33
b)
5
c)
15
d)
75
16.

Changing the number of protons in an atom will change the atom's _____

a)

color

b)

atomic weight/mass

c)

net charge

d)

identity (name of element)

17.
Calculate the atomic number of an atom with :
2 protons
3 neutrons
4 electrons
a)
2
b)
3
c)
4
d)
5
18.
Calculate the atomic weight/mass of an atom with:
11 protons
10 neutrons
11 electrons
a)
11
b)
21
c)
22
d)
10
19.
A gas
a)
has a definite shape but no definite volume
b)
has a definite volume but no definite shape
c)
has fast-moving particles
20.
Define a liquid.
a)
Indefinite shape, indefinite volume
b)
Definite shape, definite volume
c)
Found in stars
d)
Definite volume, indefinite shape
21.

The chemical bond formed when two atoms share electrons is call a(n)

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

electron bond

22.

An ionic bond is formed when

a)

Valence electrons are shared.

b)

Valence electrons surround the cations.

c)

Valence electrons are transferred between atoms.

d)

Valence electrons are completely transferred between two metals.

23.

Cations are ions with _________ charge.

a)

positive

b)

negative

c)

gains

d)

loses

24.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
25.
Is burning wood a chemical or physical change?
a)
chemical
b)
physical
26.

Is glass breaking a chemical or physical change?

a)
chemical
b)
physical
27.
Is a a rusting bicycle a chemical or physical change?
a)
chemcial
b)
physical
28.
Is melting ice a chemical or physical change?
a)
chemical
b)
physical
29.

What is the molar mass of Cl2?

a)

17 g/mol

b)

35.5 g/mo;

c)

71.0 g/mol

d)

89 g/mol

30.

What id the molar mass of UF6?

a)

101 g/mol

b)

238 g/mol

c)

257 g/mol

d)

352 g/mol

31.

Calculate the molar mass of KOH.

a)

28 g/mol

b)

56 g/mol

c)

84 g/mol

d)

112 g/mol

32.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
33.
Calculate the molarity of the following solution:  1.0 mole of KCl in 750.0 mL of solution.
a)
0.750 M
b)
99 M
c)
1.3 M
d)
2.0 M
34.
What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 500 mL?
a)
300. M
b)
31.3 M
c)
3.13 M
d)
1.56 M
35.

This type of mixture has large enough particles that you can see the different types of particles.

a)

Homogeneous

b)

Heterogeneous

c)

Colloid

d)

Solution

36.

A mixture with such small particles that you cannot see the individual particles.

a)

Suspension

b)

Sublimation

c)

Heterogeneous

d)

Homogeneous

37.

Which of the following examples is a Heterogeneous mixture?

a)

Tap Water

b)

Beach Sand

c)

Vanilla Cake Mix

d)

Bottle of Cola

38.

Which of the following examples is a Homogeneous mixture?

a)

Tap Water

b)

Beach Sand

c)

Chocolate chip cookie

d)

Mud water

39.
How many atoms of carbon (C) are in C6H12O6?
a)
3
b)
6
c)
12
d)
24
40.
Which of the following shows the correct way to balance the chemical equation?
Fe + O2 -> Fe2O3
a)
4Fe + 3O2 -> 2Fe2O3
b)
2 Fe + 3O2 -> Fe2O6
c)
4 Fe + O6 -> 2Fe2O3
d)
None of the options are correctly balanced.
41.
What is the left part of a chemical equation called?
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
42.
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 lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
43.
What is the right part of a chemical equation called...
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
44.
Balance this equation
_Al +_HCl --> _H2 +_AlCl3
a)
2, 6, 3, 2
b)
it is already balanced
c)
4, 12, 3, 4
d)
2, 1, 4, 5
45.
Balance this equation.
_Mg + _Cl2 --> _MgCl2
a)
1, 2,1
b)
already balanced
c)
2,1,1
d)
1,1,2
46.

Four substances were tested for pH, lemon juice (pH 2), baking soda (pH 9), bleach (pH 12), and milk (pH 6). Which of the following correctly lists the substances from most basic to acidic?

a)

lemon juice, milk, baking soda, bleach

b)

bleach, baking soda, milk, lemon juice

c)

milk, lemon juice, baking soda, bleach

d)

baking soda, bleach, lemon juice, milk

47.

Which of these is a property of acidic solutions?

a)

they taste sour

b)

they feel slippery

c)

they are in many cleaning products

d)

they taste bitter

48.

Neutral solutions have a pH of

a)

pH of 2

b)

pH of 0

c)

pH of 7

d)

A neutral solution does not have a pH

49.

Which is NOT a property of a base?

a)

Tastes sour

b)

Slippery

c)

Bitter taste

d)

Turns red litmus to blue

50.

What is radioactivity?

a)

An unstable atom releases energy to become stable

b)

A stable atom gains energy and becomes unstable

c)

When a bomb goes off.

d)

Negatively charged particles are emitted from the nucleus

51.

What type of decay does this symbol represent?

a)

beta decay

b)

alpha decay

c)

fission

d)

fusion

52.
This is an example of...
a)
Fission  reaction
b)
Fusion reaction
c)
Decomposition reaction
d)
Decay
53.

_____is the joining of atomic nuclei

a)

Fusion

b)

chain reaction

c)

Photosynthesis

d)

Fission

54.

Arrange in order of increasing ability to penetrate matter.

a)

Beta, gamma, alpha

b)

Alpha, gamma, beta

c)

Gamma, beta, alpha

d)

Alpha, beta, gamma

55.

emitted helium nucleus

a)

positron

b)

radioactivity

c)

alpha particle

d)

gamma radiation

e)

beta particle

56.

After one ____________ of a radioactive element, half of the original radioactive material remains.

a)

half-life

b)

cycle

c)

decay

57.

Three types of nuclear radiation are _______ radiation, _________radiation, and _____________ radiation.

a)

alpha, beta, and gamma

b)

theta, beta, and kappa

c)

alpha, beta, positron

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