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Worksheets

HC: Fall Semester Review Part 2 (2023)

Total questions: 224

Worksheet time: 4hrs 44mins

Name
Class
Date
1.

Which of these determines the identity of an atom?

a)

proton

b)

neutron

c)

valence electron

d)

protons and neutrons

2.

Gaining or losing neutrons in an atom changes its (a)   .

Choose from the below words
isotope type
charge
identity. It becomes a different element
3.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
4.

Gaining or losing protons in an atom changes its (a)   .

Choose from the below words
identity. It becomes a different element
charge
isotope type
5.

In the given notation, what does 289 represent?

a)

mass number

b)

atomic number

c)

number of neutrons

d)

number of electrons

e)

number of protons

6.

How many neutrons does this isotope of titanium have?

a)

48

b)

22

c)

26

d)

70

7.

Gaining or losing electrons in an atom changes its (a)  

Choose from the below words
idenidentity. It becomes a different element
charge
isotope type
8.

The name of this isotope of titanium is

a)

titanium-48

b)

titanium-22

c)

titanium-26

9.

Iodine-129 has _ protons

(a)  

10.

Iodine-129 has _ neutrons



(a)  

11.

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  

12.

In the given notation, what does 115 represent for the atom? (Select all that apply.)

a)

mass number

b)

atomic number

c)

number of neutrons

d)

number of protons

13.

The mass number of an atom is calculated by adding the (a)   with the protons.

Choose from the below words
neutrons
electrons
atomic mass
atomic number
14.

The name of the isotope for the given element is chromium- (a)   .

Choose from the below words
52
24
21
28
3+
15.

There are ​ (a)   protons in the given element.

Choose from the below words
24
52
21
28
16.

There are ​ (a)   electrons in the given element.

Choose from the below words
24
52
21
28
17.

There are ​ (a)   neutrons in the given element.

Choose from the below words
24
52
21
28
18.

Label each part of the symbol notation.

a)

mass number

b)

atomic number

c)

element symbol

1
2
3
1)
2)
3)
19.

What is the charge of the ion for phosphorus that has 18 electrons?

a)

3-

b)

3+

c)

1-

d)

1+

20.

What is the charge of the ion for calcium that has 18 electrons?

a)

2+

b)

2-

c)

1-

d)

1+

21.

The charge of an ion is determined by subtracting the number of ​ (a)   minus the number of ​ (b)   .​

Choose from the below words
protons
electrons
neutrons
atomic mass
mass number
22.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
23.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
24.

What element does this Bohr diagram represent?

a)

Helium

b)

Oxygen

c)

Sodium

d)

Phosphorous

25.
This is the correct dot diagram for nitrogen (N)
a)
true
b)
false
26.
This is a correct dot diagram for magnesium (Mg)
a)
true
b)
false
27.
This is a correct dot diagram for carbon (C)
a)
true
b)
false
28.
This is a correct dot diagram for nitrogen (N)
a)
true
b)
false
29.

What is the term that describes the amount of energy required to remove an electron from an atom?

a)

ionization energy

b)

electronegativity

c)

atomic radius

d)

octet rule

30.
This is a correct dot diagram for neon (Ne)
a)
true
b)
false
31.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
32.

What element is best represented by the given Bohr diagram?

a)

Boron

b)

Carbon

c)

Nitrogen

d)

Lithium

33.
What element is represented in this Bohr Model? 
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
34.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
35.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
36.
What is the name of the group that never reacts--ever ever they are stable with a full outermost ring!!!
a)
noble gases
b)
transition
c)
halogens
d)
borons
37.
Isotopes are elements with a different amount of
a)
protons
b)
neutrons
c)
electrons
d)
atoms
38.

Which period is bromine located?

a)

3

b)

17

c)

4

d)

16

39.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
40.

Choose the chemical property.

a)

brown color

b)

solid state of matter

c)

reacts with hydrogen

d)

melting point 342K

41.

Which state of matter has particles packed together in fixed positions?

a)

solid

b)

liquid

c)

gas

d)

plasma

42.

Which state of matter has particles spread far apart that can be most easily compressed?

a)

solid

b)

liquid

c)

gas

43.
This could be the dot diagram of
a)
O
b)
B
c)
Li
d)
Ne
44.

Who developed the model of the atom showing that electrons reside in energy shells?

a)

Ruthorford

b)

Bohr

c)

Thomson

d)

Dalton

45.

As you move down group, what happens to atomic radii?

a)

stays the same size

b)

size increases, decreases, then increases again

c)

increases in size

d)

decreases in size

46.

What is the term that describes an elements ability to attract electrons when bonded?

a)

ionization energy

b)

electronegativity

c)

octet rule

d)

ionic radius

47.

Which of the following causes a line emission spectrum to be seen?

a)

b)

48.

Which trend is represented in the provided image?

a)

increasing electronegativity

b)

increasing ionization energy

c)

increasing atomic radius

d)

increasing ionic radius

49.

What is the unknown?

a)

aluminum

b)

lithium

c)

lithium and aluminum

d)

aluminum and magnesium

50.

What is the highest energy level for elements in period 5?

a)

2

b)

3

c)

4

d)

5

51.

What is the trend for increasing electronegativity?

a)

Period: left to right

Group: top to bottom

b)

Period: right to left

Group: top to bottom

c)

Period: left to right

Group: bottom to top

d)

Period: right to left

Group: bottom to top

52.

An atom or group of atoms that has a positive or negative charge.

a)

atom

b)

molecule

c)

ion

d)

quark

53.

A positively charged ion. Becomes smaller than the neutral atom.

a)

cation

b)

anion

54.

A negatively charged ion. Becomes larger than the neutral atom.

a)

cation

b)

anion

55.

A horizontal row of elements in the periodic table

a)

family

b)

column

c)

group

d)

period

56.

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

a)

rows

b)

periods

c)

groups

d)

trends

57.

What are the main group elements?

a)

groups 3-12, 18

b)

groups 1, 2, 13-18

c)

periods 1-2

d)

periods 3-6

58.

Reorder the following in the proper order for color to be seen.

a)

Electron in it ground state

b)

Photon hits electron.

c)

Transferred energy sends electron to a higher energy level.

d)

Electron is in an excited state.

e)

Electron returns toward ground state, emitting absorbed energy.

1)
2)
3)
4)
5)
59.

States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons

a)

rule of 8

b)

octet rule

c)

noble gas rule

d)

magic 8

60.

groups 3-12 on the periodic table

a)

metalloids

b)

alkali metals

c)

alkaline earth metals

d)

transition metals

61.

Which of the following represents the element with the smallest radius?

a)

Rb+Rb^+  

b)

RbRb  

c)

KrKr  

d)

Se2−Se^{2-}  

62.

Most of the elements on the periodic table are classified as (a)   .

Choose from the below words
metals
Nonmetalsn
metalloids
periods
63.
This class of elements are sometimes called "semiconductors."
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Groups
64.

Metals are found on the ​ (a)   side of the periodic table.

Choose from the below words

nonmetals

right

metals

left
65.

What is the organizational system or chart for elements?

a)

Atomic weight

b)

Families

c)

Periodic table

d)

Atomic number

66.

What do you call the horizontal row of elements in a periodic table of elements?

a)

Group

b)

Family

c)

Period

d)

Column

67.

How many groups and periods does a Periodic Table have?

a)

There are 17 groups and 7 periods.

b)

There are 18 groups and 7 periods.

c)

There are 7 groups and 18 periods.

d)

There are 18 groups and 6 periods

68.

Which of the following are the three major groups of elements in the periodic table?

a)

Metals, non-metals, metalloids

b)

Metals, conductors, metalloids

c)

Metals, conductors, insulators

d)

Non-metals, conductors, insulators

69.

What are Group 1 elements known as?

a)

Alkali metals

b)

Transition elements

c)

Alkaline earth metals

d)

Inner transition elements

70.

The following elements belong to the same group EXCEPT?

a)

Argon

b)

Calcium

c)

Helium

d)

Krypton

71.

What does the C represent?

a)

atomic mass

b)

atomic number

c)

element name

d)

chemical symbol

72.

What does the 6 represent?

a)

atomic mass

b)

atomic number

c)

element name

d)

chemical symbol

73.

What does 12.011 represent?

a)

atomic mass

b)

atomic number

c)

element name

d)

chemical symbol

74.

The modern Periodic Table of Elements is arranged by (a)   .

Choose from the below words

atomic mass

atomic number

valence electrons

number of isotopes

75.

Which family of the periodic table is Neon a part?

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

76.

Which is a halogen?

a)

Helium

b)

Chlorine

c)

Oxygen

d)

Neptune

77.

I am a nonmetal

I am in period 2

I am in group 16

a)

Ba

b)

Si

c)

O

d)

S

78.

I am a metal

I am in group 2

I am in period 6

I am…

a)

Mo

b)

Re

c)

S

d)

Ba

79.
How many protons are in this element?
a)
79
b)
196
c)
117
d)
Cannot be determined
80.

Who invented the Periodic Table?

a)

Mendeleev

b)

Bohr

c)

Lewis

d)

Democritus

81.

Label each of the areas on the periodic table with the types of elements found in the periodic table.

a)

Metals

b)

Metalloids

c)

Nonmetals

1
2
3
1)
2)
3)
82.

Which of the following elements are liquids at room temperature?

A
B
C
D
E
F
G
83.

Which of the following elements are gases at room temperature?

A
B
C
D
E
F
G
84.

Which of the following elements are solids at room temperature?

A
B
C
D
E
F
G
85.

Which of the following elements diatomic?

A
B
C
D
E
F
G
H
86.

Which family are the halogens?

A
B
C
D
87.

Which family are the transitions metals?

A
B
C
D
88.

Which family are the alkali metals?

A
B
C
D
89.

Which family are the noble gases?

A
B
C
D
90.

Which family are made up of gases, liquids and solids?

A
B
C
D
91.

Which family are made up only metals?

A
B
C
D
92.

Which has the greater electronegativity: 
Cl or Al?

a)
Cl
b)
Al
93.

Which has the greater electronegativity: 
N or C?

a)
C
b)
N
94.

Which has the greater electronegativity: 
H or F?

a)
H
b)
F
95.

Which of the following will have a larger atomic radius than Zinc?

a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
96.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
97.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
98.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
99.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
100.

As you move down the periodic table the atomic radius gets bigger.  This is because ____________.

a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
101.

As you move across the periodic table the atomic radius tends to get smaller because, ______________.

a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
102.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
103.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
104.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
105.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
106.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
107.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
108.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

109.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
110.

Atomic radius generally increases as we move __________.  

a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
111.

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
112.

Which of the following will have similar properties to 1s2 2s2 2p6 3s2 3p2?

a)

carbon

b)

calcium

c)

chlorine

d)

cesium

113.

What is the electron configuration for potassium?

a)

1s2 2s2 2p6 3s2 3p6 4s1

b)

1s2 2s2 2p6 3s2 3p6 4s2

c)

1s2 2s1 2p6 3s2 3p5 4s1

d)

1s2 2s2 2p6 3s1

114.

What electron configuration matches an oxygen atom?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

115.

Identify the Electron Configuration for Aluminum (Al)

a)

1s2 2s2 2p6 3s2 3p1

b)

1s2 2s2 2p6 3s2 3p3

c)

1s2 2s2 2p6 3s2 4p1

116.

What is the position of an element in the periodic table if its electron configuration is 1s2 2s2 2p6 3s2 3p5?

a)

Group 1

b)

Group 2

c)

Group 15

d)

Group 17

117.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
118.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
119.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
120.

What is the noble gas notation electron for Sulfur?

a)

[Ne] 3p4

b)

[He] 3s2 3p4

c)

[Ne] 3s2 3p4

d)

[Na] 3s2 3p4

121.

What is the noble gas notation for V?

a)

[Ar] 4s2 4d2

b)

[Kr] 4s2 3d3

c)

[Ar] 4s2 4d3

d)

[Ar] 4s2 3d3

122.

What is the noble gas configuration for silicon?

a)

[Ne] 3s2 3p1

b)

[Ar] 4s1

c)

[Kr] 5s1

d)

[Ne] 3s2 3p2

123.
Question Image

Match the parts of the electron configuration to what it represents.

a)

1

1.

period

b)

s

2.

block

c)

2

3.

element

124.

Finish the electron configuration for chlorine:

1s2 2s2 (a)   3s2 3p6

125.

Match the group to the configuration that it ends with.

a)

s1

1.

alkali metals

b)

s2

2.

alkaline earth metals

c)

p5

3.

halogens

d)

p6

4.

noble gases

126.

This element's electron configuration got mixed up! What element is this?

x6 x2 x10 x6 x6 x2 x2 x2 x9 x2

(a)  

127.

What is the missing piece?

1s2 2s2 ___ 3s1

a)

2p6

b)

2p4

c)

3p6

d)

3s2

128.

What are the missing pieces?

1s2 2s2 2p6 ___ 3p6 4s2 ___ 4p2

a)

3s2 , 4d10

b)

2p4 , 3d10

c)

3p6 , 3d10

d)

3s2 , 3d10

129.

Match the element to it's noble gas notation:

a)

krypton

1.

[Kr]

b)

silicon

2.

[Ne] 3s2 3p2

c)

strontium

3.

[Kr] 5s2

d)

copper

4.

[Ar] 4s2 3d9

130.

Place the terms in the correct order to for an electron configuration.

a)

1s2

b)

2s2

c)

2p6

d)

3s2

e)

3p6

1)
2)
3)
4)
5)
131.

Reorder these from shortest electron configuration to the longest:

a)

hydrogen

b)

boron

c)

argon

d)

calcium

e)

xenon

1)
2)
3)
4)
5)
132.

What is orbital notation?

a)

A method of visualizing the movement of planets in the solar system.

b)

A technique for mapping the trajectory of a satellite in space.

c)

A system for representing the arrangement of atoms in a molecule.

d)

A way of representing the electron configuration of an atom using arrows and numbers.

133.

What is an orbital filling diagram?

a)

A diagram showing the movement of planets in the solar system.

b)

A diagram illustrating the structure of an atom.

c)

A diagram representing the arrangement of protons and neutrons in the nucleus of an atom.

d)

A visual representation of the arrangement of electrons in the orbitals of an atom or ion.

134.

How are electrons represented in an orbital filling diagram?

a)

Numbers

b)

Arrows pointing left or right

c)

Colors

d)

Arrows pointing up or down

135.

What is the maximum number of electrons that can occupy an s orbital?

a)

2

b)

6

c)

4

d)

8

136.

What is the maximum number of electrons that can occupy the p orbitals?

a)

6

b)

8

c)

4

d)

2

137.

What is the maximum number of electrons that can occupy the d orbitals?

a)

2

b)

10

c)

6

d)

4

138.

What is the maximum number of electrons that can occupy the f orbitals?

a)

10

b)

14

c)

6

d)

2

139.

How many orbitals are there in the p sublevel?

a)

5

b)

1

c)

3

d)

7

140.

How many orbitals are there in the d sublevel?

a)

5

b)

2

c)

8

d)

10

141.

How many orbitals are there in the f sublevel?

a)

7

b)

5

c)

3

d)

9

142.

How are orbitals represented in an electron orbital diagram?

a)

Numbers

b)

Arrows pointing left or right

c)

Letters

d)

Arrows pointing up or down

143.

How are energy levels represented in an electron orbital diagram?

a)

Numbers

b)

Arrows pointing left or right

c)

Letters

d)

Arrows pointing up or down

144.

Which subatomic particles have a positive charge?

a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
145.

Select each of the options that describes the nucleus.

a)

positively charged

b)

very dense

c)

contains the majority of mass

d)

contains the majority of the space

e)

orbits the atom

146.

​ (a)   discovered the electron within the atom.

Choose from the below words
James Chadwick 
Ernest Rutherford
John Dalton
JJ Thomson
147.

The Gold Foil Experiment was used by (a)   when he discovered the existence of the nucleus.

Choose from the below words
Ernest Rutherford
James Chadwick
JJ Thomson
John Dalton
148.

The neutron was discovered by (a)   .

Choose from the below words
James Chadwick
John Dalton
Ernest Rutherford
JJ Thomson
149.

Which these subatomic particles have a mass roughly equal to 1 amu?

a)

protons

b)

electrons

c)

neutrons

d)

nucleus

150.
Which is an electron?
a)
A
b)
B
c)
C
151.
Which item on this element square is the chemical symbol?
a)
Copper
b)
29
c)
Cu
d)
63.546
152.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
153.
An atom of the element with atomic number 6 always has _____.
a)
six protons in its nucleus
b)
an atomic mass of six
c)
more than six neutrons
d)
six electron clouds
154.

Which of the following are subatomic particles?

a)
the nucleus 
b)
electron cloud
c)

neutrons

d)

electrons

e)

protons

155.
How many protons does an atom with an atomic number of 28 and a mass number of 40 have?
a)
28
b)
68
c)
12
d)
40
156.
The following picture represents which atomic model?
a)
JJ Thomson
b)
John Dalton
c)
Ernest Rutherford
d)
Schrodinger & Heisenberg
157.
The following picture represents which atomic model?
a)

James Chadwick

b)
Democritus
c)

Ernest Rutherford

d)
JJ Thomson
158.

What subatomic particle has a neutral charge?

a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
159.

Reorder the following in proper chronological order.

a)

b)

c)

d)

e)

1)
2)
3)
4)
5)
160.

Organize these options into the right categories.

Categorize the following

neutron

atomic theory

nucleus

electron

JJ Thomson
Ernest Rutherford
John Dalton
James Chadwick
161.

How many quantum numbers are needed to describe the energy state (the "address") of an electron in an atom?

a)
1
b)
2
c)
3
d)
4
162.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
163.
The angular momentum quantum number indicates the (a)  
Choose from the below words
orientation an orbital around the nucleus.
shape of an orbital.
direction of the spin of the electron in its orbital.
main energy level of an orbital.
164.

An electron for which n=4 has more ​ (a)   than an electron for which n=2.

Choose from the below words
spin
particle nature
wave nature
energy
165.

Which of the following is used for calculating the average atomic mass of an element?

a)

Σ% abuundance x atomic mass\Sigma\%\ abuundance\ x\ atomic\ mass

b)

E=hνE=h\nu

c)

c = νλc\ =\ \nu\lambda

d)

massvolume\frac{mass}{volume}

166.
The set of orbitals that are dumbbell shaped and directed along the x, y, and z axes are called  (a)  
Choose from the below words
d orbitals.
p orbitals.
f orbitals.
s orbitals.
167.

Organize these options into the right categories.

Categorize the following

can hold 2 electrons

has 3 orientations

has 5 orientations

can hold 14 electrons

first occurs in the 3rd energy level

first occurs in the 4th energy level

occurs in every energy level

s orbital
p orbital
d orbital
f orbital
168.

The second primary quantum number contains a total of ​ (a)   orbitals.

Choose from the below words
two
three
eight
four
169.
How many orientations can an d orbital have about the nucleus?
a)
1
b)
2
c)
3
d)
5
170.

The distance traveled between two successive peaks of a waves is the (a)  

Choose from the below words
speed.
frequency.
wavelength.
energy.
171.

A line spectrum is produced when an electron moves from one energy level
(a)  

Choose from the below words
into the nucleus.
to another position in the same sublevel.
to a higher energy level.
to a lower energy level.
172.
If electrons in an atom have the lowest possible energies, the atom is in the
a)
ground state.
b)
inert state.
c)
excited state.
d)
radiation-emitting state.
173.

Which of the given orbitals can never exist according to the quantum description of an atom?

a)
6d.
b)
3f.
c)
3d.
d)
8s.
174.

According to the Bohr model of the atom, the single electron of a hydrogen atom circles the nucleus (a)  

Choose from the below words
in specific, allowed orbits.
in one fixed orbit at all times.
at any of an infinite number of distances, depending on its energy.
counterclockwise.
175.

What is the difference between the 1s and the 2s energy orbital?

a)

The shape of the orbital.

b)

The size of the orbital.

c)

The number of electrons it can hold.

d)

The number of orientations.

176.

Which of the following values does NOT represent a valid electron?

a)

n=2, l= 1, ml=1, ms=+1/2

b)

n=4, l= 2, ml=-1, ms=-1/2

c)

n=2, l= 0, ml=0, ms=-1/2

d)

n=4, l= 2, ml=-3, ms=+1/2

177.

Which form of radiation has the highest frequency?

a)

radio waves

b)

ultraviolet

c)

x-ray

d)

gamma

178.

The equation the relates the wavelength and the frequency is (a)   , in which the constant is ​ (b)   and has a value of ​ (c)   .

Choose from the below words
c = νλ
E = hν
speed of light
3.00 x 10⁸
Planck's constant
6.626 x 10⁻³⁴
179.

The orbital notation in the image represents the electrons for the element (a)   .

180.

The quantum address for the 23rd electron in the orbital notation in the image is (a)   .

181.

Indicate the respective coefficients needed to balance the chemical equation.

N2O5(s) + NO(g) → NO2(g)

(a)  

182.

Indicate the respective coefficients needed to balance the chemical equation.

Si2H3(s) + O2(g) → SiO2(s) + H2O(l)

(a)  

183.

Indicate the respective coefficients needed to balance the chemical equation.

SiCl4(s) + H2O(l) → H4SiO4(s) + HCl(l)

(a)  

184.

Indicate the respective coefficients needed to balance the chemical equation.

NaOH(aq) + Cl2(aq) → NaCl(aq) + NaClO(aq) + H2O(l)

(a)  

185.

Indicate the respective coefficients needed to balance the chemical equation.

NO2(g) + H2O(l) → HNO3(aq) + NO(g)

(a)  

186.

Indicate the respective coefficients needed to balance the chemical equation.

              K2CrO4(aq) + Fe(NO3)3(aq) → Fe2(CrO4)3↓ + KNO3(aq)

(a)  

187.

Indicate the respective coefficients needed to balance the chemical equation.

Mg(s) + Cr2(SO4)3(aq) → MgSO4(aq) + Cr(s)

(a)  

188.

Indicate the respective coefficients needed to balance the chemical equation.

NaCl(aq) + H2O(l) → NaOH(aq) + H2(g) + Cl2(g)

(a)  

189.

Indicate the respective coefficients needed to balance the chemical equation.

C2H6(g) + O2(g) → H2O(l) + CO2(g)

(a)  

190.

Indicate the respective coefficients needed to balance the chemical equation.

Cl2(g) + CH4(g) → CCl4(l) + HCl(s)

(a)  

191.

Indicate the respective coefficients needed to balance the chemical equation.

Zn(s) + HCl(aq ) → ZnCl2(aq) + H2(g)

(a)  

192.

Indicate the respective coefficients needed to balance the chemical equation.

Rb(s) + H2O(l) → RbOH(aq) + H2(g)

(a)  

193.

Indicate the respective coefficients needed to balance the chemical equation.

Ba(s) + O2(g) → BaO(s)

(a)  

194.

Indicate the respective coefficients needed to balance the chemical equation.

SiCl4(s) + H2O(l) → SiO2(s) + HCl(aq)

(a)  

195.

Indicate the respective coefficients needed to balance the chemical equation.

Sb(s) + I2(s) → SbI3(s)

(a)  

196.

Indicate the respective coefficients needed to balance the chemical equation.

NO(g) + O2(g) → NO2(g)

(a)  

197.

Indicate the respective coefficients needed to balance the chemical equation.

H2(g) + N2(g) → NH3(l)

(a)  

198.

Indicate the respective coefficients needed to balance the chemical equation.

C(s) + H2O(l) → CO(g) + H2(g)

(a)  

199.

Indicate the respective coefficients needed to balance the chemical equation.

Na(s) + Cl2(g) → NaCl(s)

(a)  

200.

Indicate the respective coefficients needed to balance the chemical equation.

Mg(s) + H2O(l) → Mg(OH)2(aq) + H2(g)

(a)  

201.

WHat is the type of bond in which the valence electrons are free to move throughout the substance?

a)

ionic

b)

molecular covalent

c)

metallic

d)

network covalent

202.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
203.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
204.

An ionic bond forms when (a)   .

Choose from the below words
valence electrons are shared
a sea of mobile electrons surround the cations
valence electrons are transferred between atoms
none of the above
205.
Predict the bond that will form between Be and F.
a)
Ionic
b)

Covalent

c)

Metallic

206.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)

Covalent

c)

Metallic

207.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
c)

Metallic

208.
What is a valence electron?
a)

An electron that is found in the outermost shell of an atom. 

b)

An electron found in the innermost shell of an atom.

c)

An electron found in the middle shell.

d)

All electrons within an atom.

209.

A (a)   is formed between atoms when electrons are shared.

Choose from the below words
chemical bond
covalent bond
oxidation #
ionic bond
210.

What type of substance is a brittle solid that conducts electricity when dissolved in water?

a)

network covalent

b)

metallic

c)

molecular covalent

d)

ionic

211.

What type of substance is a bendable hard solid that conducts electricity but does not dissolve in water?

a)

network covalent

b)

ionic

c)

metallic

d)

molecular covalent

212.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
213.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
214.

Which of the following is NOT a property of ionic compound?

a)

Solid at room

temperature

b)

Insoluble in water

c)

Molten ionic

compounds

conduct

electricity

 

d)

High melting &

boiling point

215.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
216.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
217.

In the correct Lewis structure for methane, CH4, how many unshared electron pairs surround the carbon?

a)
2
b)
8
c)
0
d)
4
218.

In carbon dioxide, CO2, how many UNSHARED pairs of electrons does each oxygen have?

a)
2
b)
1
c)
4
d)
6
219.

3. Which is a correct Lewis structure for hydrogen cyanide, HCN?

a)
b)
c)
d)
220.

How many electrons can be used in the Lewis Structure for : NO3-

a)
23
b)
20
c)
18
d)
24
221.

How many electrons are represented by each line in a shared bond??

a)
1
b)
2
c)
3
d)
4
222.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
223.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
224.

Which of these is the correct Lewis structure for SiBr4?

a)

A

b)

B

c)

C

d)

D

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