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24-25 IB MYP Chemistry Unit 1 Review

Total questions: 95

Worksheet time: 2hrs 41mins

Name
Class
Date
1.

Which of the following is a homogeneous mixture?

a)

Colloid

b)

Suspension

c)

Solution

d)

Compound

2.

What is used to calculate the average atomic mass of an element?

a)

Mass spectroscopy

b)

Chemical reactions

c)

Physical measurements

d)

Visual inspection

3.

What are the three main types of radioactive decay?

a)

Alpha, beta, and gamma decay

b)

Delta, epsilon, and zeta decay

c)

Sigma, tau, and omega decay

d)

Muon, pion, and kaon decay

4.

What type of mixture is a snow globe?

a)

Homogeneous

b)

Element

c)

Heterogeneous

d)

Compound

5.

What is the charge of a neutron?

a)

Neutral

b)

Positive

c)

Negative

d)

Variable

6.

What is the atomic number of Neon as shown in the diagram?

a)

10

b)

20

c)

2

d)

4

7.

What is the atomic number of Cobalt?

a)

27

b)

28

c)

26

d)

29

8.

Which of the following is NOT a type of nuclear decay?

a)

Alpha decay

b)

Beta decay

c)

Gamma decay

d)

Delta decay

9.

What is the relative abundance of the Ge - 76?

a)

21.22%

b)

36.52%

c)

7.75%

d)

100%

10.

How many electrons does Phosphorus have?

a)

A. 15

b)

B. 16

c)

C. 31

d)

D. 46

11.

The atomic mass of an atom is equal to

a)

number of protons plus number of neutrons

b)

number of protons plus number of electrons

c)

number of electrons plus the number of neutrons

12.
What is the mass of an atom if it has 11 protons, 12 neutrons, and 11 electrons?
a)
22
b)
11
c)
34
d)
23
13.
If a sulfur atom has 16 protons, 16 electrons, and 16 neutrons, its atomic mass is:
a)
16
b)
32
c)
48
d)
64
14.

Positively charged particle found in the nucleus. They determine the identity of an element and makeup half of an atom’s mass.

(a)  

15.

A neutrally charged particle that is found in the nucleus. They are important for the stability of the nucleus. It makes up the other half of the atom’s mass.

(a)  

16.

The smallest subatomic particle that has a negative charge. These orbit outside of the nucleus and are important in how an atom bonds with other atoms.

(a)  

17.

The center area of an atom containing the protons and neutrons.

(a)  

18.

A substance made up of all the same types of atoms. EX: A piece of pure carbon is made up of only carbon atoms.

(a)  

19.

Atoms of the same element with different numbers of neutrons.

(a)  

20.

What is the main difference between a compound and an element?

a)

Both are pure substances

b)

Compounds can be physically separated

c)

Elements are formed by two or more elements chemically joined together

d)

Compounds cannot be divided into simpler substances

21.

Which of the following is a characteristic of a homogeneous mixture?

a)

Visibly different components

b)

Uniform throughout the mixture

c)

Cannot be physically separated

d)

Formed by two or more elements chemically joined together

22.

Which of the following is an example of a heterogeneous mixture?

a)

Salt water

b)

Mouthwash

c)

Vegetable soup

d)

Smooth peanut butter

23.

Where are electrons located in an atom?

a)

In the central nucleus

b)

In the electron clouds surrounding the nucleus

c)

Within the neutron

d)

In the outermost energy level

24.

What is the atomic number of an element?

a)

The number of protons in an element

b)

The number of protons and neutrons in an element

c)

The number of total electrons in a neutral atom

d)

The identity of an element

25.

What does it mean for an atom to be electronically neutral?

a)

It has an equal number of protons and electrons

b)

It has an equal number of protons and neutrons

c)

It has an equal number of electrons and neutrons

d)

It has a total charge of zero

26.
This is how you find the number of neutrons in an atom. 
a)
Subtract the atomic number from the atomic mass
b)
Subtract the atomic mass from the atomic number 
c)
Add the atomic mass to the atomic number 
d)
Divide the atomic mass by the atomic number 
27.

Who proposed that electrons move around the nucleus in distinct circular orbits?

a)

Bohr

b)

Rutherford

c)

Chadwick

d)

Thomson

28.

This picture best represents ___________________ atomic model.

a)

Thomson's

b)

Dalton's

c)

Bohr's

d)

Chadwick's

29.
In Dalton's Atomic Theory, all elements consist of __________ that cannot be divided.
a)
Atoms
b)
Parts
c)
Molecules
d)
Hydrogen
30.

Which of the following is/are conclusions based on Rutherford’s gold foil experiment?

a)

Atom is mostly empty space

b)

The nucleus is positively charged

c)

The atom has a small dense nucleus

d)

All answers are correct

31.

Which one of these is Dalton's Model?

a)
b)
c)
d)
32.

Which model was created after the discovery of the nucleus?

a)

Dalton's

b)

Rutherford's

c)

Quantum Mechanical

d)

Plum Pudding

33.

Who discovered electrons?

a)

Rutherford

b)

Bohr

c)

J.J. Thompson

d)

Democritus

34.
Ernest Rutherford discovered that the atom was mostly _________________ and has a _______________ charged nucleus.
a)
empty space, positively
b)
empty space, negatively
c)
full of protons, positively
d)
full of neutrons, negatively
35.

Which experiment was performed by J. J. Thomson in 1897?

a)
Oil Drop Experiment
b)
Gold Foil Experiment
c)
Wave  Experiment
d)
Cathode Ray Experiment
36.
Which subatomic particle was discovered as a result of the cathode ray experiment?
a)
proton
b)
neutron
c)
electron
d)
nucleus
37.

What is the correct order of scientists in order of their work related to the atomic theory from earliest to most recent?

a)

Neils Bohr, Ernest Rutherford, JJ Thomson, John Dalton, & Democritus

b)

JJ Thomson, John Dalton, Neils Bohr, Ernest Rutherford, & Democritus

c)

Democritus, John Dalton, JJ Thomson, Ernest Rutherford, and Neils Bohr

d)

John Dalton, Neils Bohr, JJ Thomson, Democritus, & Ernest Rutherford

38.

Who proposed that electrons move around the nucleus in circular orbits?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

39.
a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

40.
a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

41.
Which of the following are made from a combination of 2 or more elements?
a)
Molecules
b)
Pure Substances
c)
Compounds
d)
Elements
42.
A homogeneous mixture of particles so small that they can not be seen with a microscope and that will never settle to the bottom of their container
a)
colloid
b)
solution
c)
suspension
d)
tyndall effect
43.
Air is what type of mixture?
a)
Heterogeneous
b)
homogeneous
c)
Compound
44.
A mixture that is NOT evenly distributed is called ....
a)
Compounded
b)
Homogenous
c)
Heterogenous
d)
Salty
45.
All matter is made up of .....
a)
Compounds
b)
Atoms
c)
Molecules
d)
Sunshine
46.
A substance with two or more elements that are combined in a fixed proportion
a)
colloid
b)
compound
c)
element
d)
solution
47.

True or False: Elements and compounds are pure substances.

a)

True

b)

False

48.
Something that takes up space and has mass.
a)
volume
b)
matter
c)
mass
d)
density
49.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
50.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
51.
What quantities vary between isotopes of an element?
a)
protons, electrons, and atomic mass
b)
protons, electrons, and atomic number
c)
neutrons and electrons
d)
neutrons and atomic mass
52.
Four isotopes of lead include lead-204, lead-206, lead-207, and lead-208.  The average atomic mass of lead is 207.2.  Which isotope of lead is likely to be the most abundant.
a)
204
b)
206
c)
207
d)
208
53.
What is the name of the pictured isotope?
a)
Chlorine-Schmorine
b)
Chlorine-17
c)
Chlorine-35
d)
Chlorine-18
54.

If X is the symbol for an element, select the two symbols represent isotopes of the same element.

a)

7735X77_{35}X   

b)

7937X79_{37}X   

c)

8136X81_{36}X  

d)

8135X81_{35}X  

55.

24.1% of all the isotopes of an element have a mass of 75.23 u, 48.7% have a mass of 74.61 u, and 27.2% have a mass of 75.20 u.

What is the average atomic mass of this element?

a)

74.92 u

b)

24.97 u

c)

75.01 u

d)

74.51 u

56.

An element has three different isotopes. One has a mass of 35.00 u; another has a mass of 36.00 u; and another has a mass of 38.00 u. What is the average atomic mass of this element?

a)
36.33 amu
b)
37.00 amu
c)
12.11 amu
d)
impossible to tell
57.
What do these isotopes of carbon all have in common?
a)

neutron number and mass number

b)

atomic number and neutron amount

c)

atomic number and electron number

d)

protons, atomic number, and mass number

58.

There are two primary isotopes found in any sample of copper: copper-63 and copper-65. The isotope 65Cu composes 69.2% of the sample and 63Cu comprises the other 30.8%. Based on this data, what is the atomic mass of copper?

a)

29 amu

b)

63.546 amu

c)

64.4 amu

d)

63.6 amu

59.

Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium?

a)

85.468 amu

b)

37 amu

c)

85.6 amu

d)

86.4 amu

60.

Isotopes are atoms of the same element with different #’s of __________ & therefore, different __________.

a)

neutrons ; atomic numbers

b)

protons ; atomic numbers

c)

electrons ; mass numbers

d)

neutrons ; mass numbers

61.

Isotopes have identical chemical properties because they have the same number of protons and electrons.

a)

True

b)

False

62.

Isotopes have identical physical properties because they have the same number of neutrons.

a)

True

b)

False

63.

How is the alpha particle written in a nuclear equation?

a)

42He

b)

24He

c)

0-1e

d)

00γ

64.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
65.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
66.

Gamma rays have

a)

no mass

b)

a huge mass

c)

a small mass

d)

an average mass

67.
Solve this equation for beta decay.
614C = ___ + -10e
a)
410Be
b)
714N
c)
210He
d)
613C
68.
Has the symbol
a)
Alpha
b)
Beta 
c)
Gamma
69.
Has the highest penetrating power.  Can penetrate our body.  Even several cm thick of lead or several meters thick of concrete cannot stop all of it.
a)
Alpha
b)
Beta
c)
Gamma
70.
Has the lowest penetrating power.  Can only penetrate 0.05 mm into the body and can be stopped by a piece of paper or clothing.
a)
Alpha
b)
Beta
c)
Gamma
71.
Uranium-238  decays into  Thorium-234  by emitting .........
a)
an alpha particle
b)
a beta particle
c)
gamma rays
d)
visible light
72.
The process of nuclear change in an atom of radioactive material is called... 
a)
nuclear decay
b)
nuclear mass
c)
isotopes
d)
radon
73.
Radioactive materials have unstable...
a)
electrons
b)
protons
c)
nuclei
d)
neutrons
74.
This is an example of...
a)
Fission  reaction
b)
Fusion reaction
c)
Decomposition reaction
d)
Decay
75.
Which process involves the joining of small nuclei?
a)
Beta decay
b)
Alpha decay
c)
Nuclear fission
d)
Nuclear fusion
76.
What is Half-life?
a)
The amount of time it takes for some of the nuclei in a sample of the isotope to decay
b)
The amount of time it takes for half the electrons in a sample of the isotope to decay
c)
The amount of time it takes for half the nuclei in a sample of the isotope to decay
d)
the amount of time it takes to double the nuclei in a sample of the isotope to decay
77.
The half-life of Zn-71 is 2.4 minutes. If one had 100.0 g at the beginning, how many grams would be left after 7.2 minutes has elapsed?
a)
100.0g
b)
50.0g
c)
12.5g
d)
8.5g
78.
After the third half-life, how much of the sample is left?
a)
1/2
b)
1/3
c)
1/16
d)
1/8
79.
If 10 mg of iodine 131 is given to a patient, how much is left after 24 days? The half-life of iodine-131 is 8 days.
a)
1.25mg
b)
1.25g
c)
10g
d)
10mg
80.
What is the half-life of iodine-131?
a)
32 days
b)
8 days
c)
16 days
d)
24 days
81.

The diagram shows 32 atoms.

16 of the Red are parent isotopes

16 of the Green are daughter isotopes

How many half-lives have occurred?

a)

0

b)

1

c)

2

d)

3

82.

What is the Half life of this isotope?

a)

5 seconds

b)

10 seconds

c)

15 seconds

d)

20 seconds

83.

What is the Half life of this isotope?

a)

5 seconds

b)

10 seconds

c)

15 seconds

d)

20 seconds

84.

A radioactive sample will lose half of its original radioactive nuclei after 1 half life.

a)

TRUE

b)

FALSE

85.
What do the peaks on the mass spectrum represent?
a)
anions
b)
different isotopes
c)
atoms with differing numbers of electrons
d)
numbers of electrons
86.
What do the heights of the peaks represent in the mass spectrum?
a)
number of isotopes
b)
relative abundance of each isotope
c)
average atomic mass
d)
charge:mass ratio
87.
How many isotopes are shown in this mass spectrum?
a)
1
b)
84
c)
86
d)
4
88.

Carbon has three known isotopes. Based on the average atomic mass from the periodic table, which is the most abundant?

a)
carbon-12.011
b)
carbon-12
c)
carbon-13
d)
carbon-14
89.

What ratio does the mass spectrometer detect?

a)

mass of main radical

b)

mass of molecular ion

c)

charge to mass ratio

d)

mass to charge ratio

90.
_______________ is the process by which unstable atoms emit radiation until they become stable.
a)
Radiation
b)
Chemical Reaction
c)
Radioactive Decay
d)
Isotopes
91.

Why does an atom have radioactive decay?

a)

It feels like it.

b)

Its nucleus is too large.

c)

Its nucleus is too small.

d)

To become more stable when It has an unstable nucleus.

92.

A(n) _________ is a physical combination of two or more different substances

a)

element

b)

molecule

c)

compound

d)

mixture

93.

A mixture that appears to be uniform while being stirred but separates into different phases when agitation ceases is a

a)
solvent
b)
colloid
c)
suspension
d)
solute
94.

An unknown mixture is a clear purple color.  You cannot see any distinct particles when you look at it.  You shine a light through the side of it and small particles are seen in the light.  What kind of mixture is this?

a)

Colloid

b)

Solution

c)

Suspension

95.

What is a heterogeneous mixture?

a)

A substance made of atoms that are all alike

b)

A mixture that is even throughout

c)

A mixture that is not even throughout

d)

Two or more elements chemically combined together

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