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ICP Chem Final

Total questions: 100

Worksheet time: 25hrs 0mins

Name
Class
Date
1.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

2.

What is the name of group number 2?

a)

transition metals

b)

halogens

c)

metaloids

d)

alkaline earth metals

3.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

4.

a row on the Periodic Table of Elements

a)

family

b)

period

c)

row

d)

isotope

5.
Which one of these is not a noble gas?
a)
Helium
b)
Radon
c)
Iodine
d)
Krypton
6.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
7.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
8.
The atomic number of this pictured element is
a)
28
b)
58.6934
c)
Ni
d)
Nickel
9.

How is the MODERN periodic table arranged left to right?

a)

Increasing number of neutrons

b)

Decreasing number of protons

c)

Increasing atomic mass

d)

Increasing number of protons

10.

Which elements will have similar properties?

a)

H, He, Li

b)

B, C, N

c)

N, P, As

d)

Al, Zn, Ag

11.

Which elements are in the same family or group?

a)

F, S, As

b)

Mg, K, Sr

c)

Be, Mg, Ca

d)

B, Si, As

12.

What is the atomic number of Fe?

a)

62

b)

56

c)

65

d)

26

13.

A vertical column in the periodic table, also known as a family of elements.

a)

Period

b)

Group

c)

Atomic Number

d)

Row

14.

A count of the number of protons in the atomic nucleus

a)

Atomic Number

b)

Atomic Mass

c)

Atomic Symbol

d)

Mass Number

15.

A horizontal row in the periodic table

a)

Period

b)

Group

c)

Atomic Number

d)

Column

16.

The total number of protons and neutrons within an isotope.

a)

Atomic Number

b)

Mass Number

c)

Atomic Symbol

d)

Atomic Nucleus

17.

If an atom has a charge of zero and a total mass of 1 AMU, how many NEUTRONS does it have?

a)

1

b)

0

c)

2

d)

1-

18.

What is the mass of an atom containing: 1 protons, 1 neutron, and 2 electrons?

a)

1-

b)

2

c)

3

d)

1

19.

What is the mass of an atom containing: 4 protons, 5 neutrons, and 4 electrons?

a)

8

b)

9

c)

0

d)

1+

20.

What is the mass of an atom containing: 2 protons, 2 neutrons, and 2 electrons?

a)

0

b)

2

c)

4

d)

6

21.

Which particle(s) resides in the nucleus?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Protons and Neutrons

22.

What particle exists outside of the nucleus?

a)

proton

b)

neutron

c)

electron

d)

none of the above

23.

Match the charge to each subatomic particle.

a)

Positive

1.

Proton

b)

Neutral

2.

Neutron

c)

Negative

3.

Electron

24.

Match the location of the atom to each subatomic particle

a)

Nucleus

1.

Proton

b)

Nucleus

2.

Neutron

c)

Cloud outside of nucleus

3.

Electron

25.

Match the terms to each definition.

a)

Abbreviation of element name

1.

Chemical Symbol

b)

Sum of protons and neutrons

2.

Mass Number

c)

Atom identity equal to number of protons

3.

Atomic Number

d)

Equal to the atomic number

4.

Proton

e)

Added to protons to get mass number

5.

Neutron

26.

If an atom has 4 protons, a mass of 12, and charge of +2, how many neutrons does it have?

a)

6

b)

8

c)

4

d)

2

27.

What is the charge of an atom containing: 1 protons, 1 neutron, and 2 electrons?

a)

2

b)

3

c)

0

d)

1-

28.

What is the charge of an atom containing: 5 protons, 7 neutrons, and 7 electrons?

a)

2-

b)

12

c)

0

d)

2+

29.

If an atom has 4 protons, a mass of 12, and charge of +2, how many neutrons does it have?

a)

6

b)

8

c)

4

d)

2

30.

This image shows some of the colored flames we will see in the fire lab. The color of light can show us which emission has the most energy released by the electrons. Which compound's electrons had the largest change in energy levels?

a)

Strontium

b)

Calcium

c)

Potassium

d)

Copper

31.

Which of the jumps in energy levels would create a photon emission with the most energy?

a)

n=1 to n=2

b)

n=2 to n=3

c)

n=2 to n=4

d)

n=1 to n=4

32.

Which has more energy?

a)

An electron in an excited state

b)

An electron at the ground state

c)

An electron in energy level n=1

d)

An electron that is not a valence electron

33.

In the diagram on the left, a photon is being emitted. What must have just occurred in the atom for the photon to be released?

a)

Energy was absorbed.

b)

The electron lost energy and fell an energy level.

c)

The electron jumped up to a higher energy level

d)

The electron is in the excited state.

34.

Which energy level would have electrons with the highest amount of energy?

a)

E1

b)

E2

c)

E3

d)

E4

35.

When an electron emits light

a)

the electron gets "excited" and "jumps out" away from the nucleus

b)

the electron gets "excited" and "drops back down" closer to the nucleus

c)

the electron "calms down" and "jumps out" away from the nucleus

d)

the electron "calms down" and "drops back down" closer to the nucleus

36.
Which is the most important characteristic in determining an element's chemical properties?
a)
the number of protons and neutrons in its nucleus
b)
which period it is found in
c)
the number of valence electrons it contains
d)
its outermost energy level
37.

How many valence electrons are most stable for an element in a compound (except hydrogen)?

(a)  

38.

A covalent bond is made of the 2 following kinds of elements:

a)

Metal and metal

b)

Nonmetal and nonmetal

c)

Metalloid and Metalloid

d)

Metal and nonmetal

39.

Ionic compounds are made of the two following kinds of elements:

a)

Metal and metal

b)

Nonmetal and nonmetal

c)

Metalloid and metalloid

d)

Nonmetal and metal

40.
What is a cation? 
a)
a metal with a negative (-) charge
b)
a non-metal with a negative (-) charge 
c)
a metal with a positive (+) charge 
d)
a non-metal with a positive (+) charge
41.
What is a anion? 
a)
a metal with a negative (-) charge
b)
a non-metal with a negative (-) charge 
c)
a metal with a positive (+) charge 
d)
a non-metal with a positive (+) charge
42.

What does electronegativity do as you go across a period?

a)

decrease

b)

no pattern

c)

stay the same

d)

increase

43.

Which of the following describes a valence electron?

a)

Outermost from nucleus

b)

Most energetic

c)

Determines chemical properties and bonding

d)

All options

44.

Which of the following would have 2 valence electrons

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble Gasses

45.

Which of the following elements will have 5 valence electrons?

a)

In

b)

Ge

c)

Sb

d)

Rn

e)

Cs

46.

This could be a Lewis structure of which element?

a)

Li

b)

Al

c)

C

d)

Be

47.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)

A

b)

B

c)

C

d)

D

48.

Match the ions to the correct compound name

a)

Na+ S2-

1.

sodium sulfide

b)

Be2+ Cl-

2.

beryllium chloride

c)

Na+ Se2-

3.

sodium selenide

d)

B3+ Br-

4.

boron bromide

e)

Ba2+ Cl-

5.

barium chloride

49.

Match each cation to the correct name.

a)

Sn2+

1.

tin (II)

b)

Sn4+

2.

tin (IV)

c)

Ti2+

3.

titanium (II)

d)

Ti3+

4.

titanium (III)

e)

Sb5+

5.

antimony (V)

50.

Match the ions to the correct compound name

a)

Fe2+ S2-

1.

iron (II) sulfide

b)

In3+ Cl-

2.

indium (III) chloride

c)

Sm7+ S2-

3.

samarium (VII) sulfide

d)

Os6+ Br-

4.

osmium (VI) bromide

e)

Mo4+ Cl-

5.

molybdenum (IV) chloride

51.

Match the compound names to the correct set of ions.

a)

cobalt (III) sulfite

1.

Co3+ SO32-

b)

cobalt (III) sulfate

2.

Co3+ SO42-

c)

chromium (II) hypochlorite

3.

Cr2+ ClO-

d)

chromium (II) chlorite

4.

Cr2+ ClO2-

e)

carbon carbonate

5.

C4+ CO32-

52.

Match each set of ions to the correct compound name

a)

K+ MnO4-

1.

potassium permanganate

b)

Ba2+ ClO4-

2.

barium perchlorate

c)

Pd2+ SO32-

3.

palladium (II) sulfite

d)

Be2+ CrO42-

4.

beryllium chromate

e)

Cu2+ Cr2O72-

5.

copper (II) dichromate

53.
Question Image

Match the following reactions with their types:

a)

Decomposition Reaction

1.

AB → A + B

b)

Single Displacement Reaction

2.

A + BC → AC + B

c)

Double Displacement Reaction

3.

AB + CD → AD + CB

d)

Synthesis Reaction

4.

A + B → AB

54.

Match the unique identifier to the reaction type

a)

Synthesis

1.

A single product

b)

Decomposition

2.

A single reactant

c)

Single Replacement

3.

An element by itself on BOTH sides

d)

Double Replacement

4.

All ions. No single compounds or elements

e)

Combustion

5.

O2 reactant. CO2 and H2O products only

55.

Label the parts of a chemical equation.

a)Product
b)Reactant
c)Direction Arrow
d)Coefficients
e)Chemical Formula
f)State of matter
g)Subscript
1
2
3
4
5
6
7
1)
2)
3)
4)
5)
6)
7)
56.

Balance this reaction and choose the answer with the correct coefficients

____ Na3PO4 + ____ KOH ---> ____ NaOH + ____ K3PO4

a)

1,3,3,1

b)

1,3,2,1

c)

2,3,3,1

d)

1,1,3,1

57.

Balance this reaction and choose the answer with the correct coefficients

____ RbNO3 + ____ BeF2 ----> ____ Be(NO3)2 + ____ RbF

a)

1,1,1,1

b)

1,2,1,1

c)

2,1,1,2

d)

2,1,2,1

58.

Balance the following and select the response with the correct coefficients

____ Fe + ____ Cl2 → ____ FeCl3

a)

1,1,2

b)

1,3,1

c)

2,2,3

d)

2,3,2

59.

Match the following

a)

Endothermic

1.

Energy is entering the system, something is getting warmer

b)

Exothermic

2.

Energy is exiting the system, something is getting colder

c)

Equilibrium

3.

Warmer and cooler temperatures balance out to be the same temperature

60.

Endothermic is when heat is ​ (a)   ; exothermic is when heat is ​ (b)  

Choose from the below words
absorbed
released
61.

Which of the following best describes temperature?

a)

a measure of the average kinetic energy of the particles in a sample of matter

b)

heat absorbed or released in a chemical or physical change

c)

heat energy

d)

energy of change

62.

The higher the kinetic energy of the particles in a sample of matter,

a)

the lower the temperature will be.

b)

temperature is not affected.

c)

the higher the temperature will be.

63.
Heat flows from _______ to ______ objects
a)
cooler to warmer
b)
warmer to warmer
c)
warmer to cooler
d)
cooler to cooler
64.
If two objects have different temperatures, heat will flow from the warmer object to the cooler one UNTIL ____________
a)
one reaches a temperature of zero
b)
they both have an equal temperature
c)
one runs out of energy
65.

What is defined as the heat required to raise the temperature of 1 g of a substance by 1 °C ?

a)

heat energy

b)

heat of formation

c)

specific heat

d)

heat capacity

66.
Question Image

Match the letter in the picture with the word

a)

A

1.

all solid

b)

B

2.

melting/

freezing

c)

C

3.

all liquid

d)

D

4.

vaporizing/

condensing

e)

E

5.

all gas

67.

Where on the graph is the kinetic energy remaining constant?

a)

A to B

b)

B to C

c)

C to D

d)

D to E

e)

E to F

68.

During a phase change, kinetic energy will _____ while potential energy will _____?

a)

stay the same, stay the same

b)

change, stay the same

c)

Stay the same, change

69.

label

a)

gas

b)

liquid

c)

solid

d)

heat lost

e)

melting

f)

freezing

g)

condenstation

h)

vaporization

i)

heat added

1
2
3
4
5
6
7
8
9
1)
2)
3)
4)
5)
6)
7)
8)
9)
70.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
71.
Question Image

Match the arrow to the description.

a)

energy of activated complex or transition state

1.

B

b)

activation energy of forward reaction

2.

A

c)

activation energy of reverse reaction

3.

D

d)

energy of products

4.

C

72.
What letter represents the energy of the products?
a)
A
b)
B
c)
C
d)
D
73.
What letter represents the activation energy?
a)
A
b)
B
c)
C
d)
D
74.
What is the energy of the activated complex?
a)
75 kJ
b)
225 kJ
c)
300 kJ
d)
225 kJ
75.

What is the change of the heat of the reaction (ΔH)?

a)

-40 kJ

b)

-20 kJ

c)

100 kJ

d)

60 kJ

76.

Match the force with the object they act upon

a)

Gravity

1.

planets, stars, and very large objects

b)

Electromagnetic

2.

protons and electrons

c)

Weak Nuclear

3.

quarks

d)

Strong Nuclear

4.

protons and neutrons

77.

Label the diagram with the attributes of the fundamental forces

a)Strongest Force
b)2nd Strongest Force
c)3rd Strongest Force
d)Weakest Force
e)Works only inside the nucleus
f)Works at infinite distance
1
2
3
4
5
6
1)
2)
3)
4)
5)
6)
78.

As the distance between particles increases, what happens to the strength of the nuclear force?

a)

decreases

b)

increases

c)

remains unchanged

79.

Match each particle to the correct arrow showing what stops the particle.

a)alpha
b)gamma
c)beta
1
2
3
1)
2)
3)
80.

During​ (a)   decay, a transformation takes place. A ​ (b)   turns into a ​ (c)   producing a/n ​ (d)   . The mass number does not change, but the ​ (e)   number increases turning the atom into a new element.

Choose from the below words
beta
neutron
proton
electron
atomic
gamma
alpha
81.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
82.

This is the correct equation for U-238 decay.

a)

true

b)

false

83.

Which of the following is needed to balance the nuclear equation seen?

a)

Pb-212

b)

Pb-216

c)

Rn-216

d)

Rn-220

84.
Solve this equation for beta decay.
6027Co = ___ + 0-1e
a)
5625Mn
b)
6028Ni
c)
5823V
d)
5927Co
85.
Identify the missing substance in each of the following nuclear reactions.
 _____→137 56 Ba + 0 −1 e 
a)
13755Ba
b)
13757La
c)
13856Ba
d)
137 55Cs
86.

Match each nuclear reaction equation to the type of nuclear decay

a)

1.

alpha decay

b)

2.

beta decay

c)

3.

positron emission

d)

4.

electron capture

87.

Fill in the gaps and define each type of nuclear reaction.

a)70
b)positron emission
c)e-
d)beta decay
e)Sn
f)energy
g)gamma decay
h)alpha decay
i)206
j)2
1
2
3
4
5
6
7
8
9
10
1)
2)
3)
4)
5)
6)
7)
8)
9)
10)
88.

Organize these options into the right categories

Categorize the following

Atoms combining into a larger atom

Atom splitting into smaller atoms

Releases lots of energy

Requires high temperatures and pressures to begin

Must force atoms to overcome electromagnetic force

Can become uncontrollable

Started by a neutron

Fueled by Uranium

Fueled by hydrogen

Can create nuclear fallout

Produces radioactive waste

Produces Helium

Process of current nuclear power plants

Process of the sun

Process of atomic bombs

Requires control rods

Controlled by magnets and lasers

Heats water into steam to produce electricity

Transforms fuel into a new element

Source of clean energy to replace fossil fuels

Nuclear Fission
Both
Nuclear Fusion
89.

What is Avogadro's number?

a)

6.02 x 1023

b)

1 mole

c)

600 million

d)

6.02

90.

A mole is:

a)

The SI unit for mass

b)

The SI unit for the amount of a substance

c)

The SI unit for volume

d)

The SI unit for area

91.

Which has the most particles?

a)

1 mole H2

b)

1 mole Na1+

c)

1 mole Al(OH)3

d)

These are all the same

92.
What are the units in molar mass?
a)
grams
b)
moles
c)
moles/gram
d)
grams/mole
93.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
94.
A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________
a)
ionic formula
b)
covalent formula
c)
empirical formula
d)
molecular formula
95.

Place the steps of determining an empirical formula in order.

a)

Change % to grams

b)

Convert grams to moles

c)

Divide all moles by lowest mole

d)

Use 2,3,4 rule if mole ratio is not all whole numbers

e)

Mole ratio is subscripts of empirical formula

1)
2)
3)
4)
5)
96.

Identify the components of the conversion from grams to moles as it is used in empirical formula determination.

a)% mass in grams
b)moles of molar mass
c)grams of molar mass
d)moles of element
e)molar mass
1
2
3
4
5
1)
2)
3)
4)
5)
97.

When calculating empirical formula, we convert grams of each element into moles. Which amount of moles should we divide all moles by?

A
B
C
98.

Label the components of the calculation of a molecular formula.

a)Mass ratio of the formulas
b)Molar Mass of molecular (real) formula
c)Molar Mass of empirical formula
1
2
3
1)
2)
3)
99.

Empirical Formula = CF2

Molecular formula mass = 192 g/mol

Molecular Formula = ?

a)

C4F8

b)

C8F4

c)

C3F6

d)

C2F4

100.

Match the following

a)

1.

Noble Gasses

b)

2.

Halogens

c)

3.

Transition Metals

d)

4.

Alkali Metals

e)

5.

Alkaline Earth Metals

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