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Structure of atom , Periodic table

Total questions: 216

Worksheet time: 3hrs 33mins

Name
Class
Date
1.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

2.
subatomic particles found on the outermost shell & responsible for the atom's reactivity
a)
neutrons
b)
valence electrons
c)
isotopes
d)
ions
3.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
4.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
5.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
6.
Where electrons are likely to be found as they travel around the nucleus
a)
Nucleus
b)
Electron Cloud
c)
Within a Proton
d)
Within a Neutron
7.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
8.
Arrangement of elements organized by atomic number
a)
Electron Cloud 
b)
Periodic Table 
c)
Electron Configuration
d)
None of these
9.

A horizontal row of elements in the periodic table

a)

Molecule

b)

Period

c)

Family

d)

Atom

10.

What is one way Neutrons are different from electrons?

a)

they both are negative

b)

neutrons have no charge, while electrons have a negative charge

c)

Both are in the nucleus( center of atom)

d)

Electrons are inside nucleus and neutrons are outside the nucleus.

11.

What is the atomic number?

a)

35

b)

18

c)

17

d)

52

12.

How many protons and electrons does this element have?

a)

35

b)

18

c)

17

d)

52

13.

How many neutrons does calcium have?

a)

20

b)

40

c)

60

d)

0

14.

What is the atomic mass of Arsenic?

a)

33

b)

107

c)

75

15.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

16.
An element's identity is determined by the number of
a)
electrons.
b)
protons.
c)
neutrons.
d)
valence.
17.
Which is an electron?
a)
A
b)
B
c)
C
18.
Which is a proton?
a)
A
b)
B
c)
C
19.
Which is a neutron?
a)
A
b)
B
c)
C
20.

Elements in the same group have the same

a)

Properties

b)

Number of electrons

c)

Number of protons

d)

Nucleus

21.
Which subatomic particles contribute the most to the mass of an atom?
a)
Protons, Neutrons, Electrons
b)
Protons only
c)
Protons and Electrons
d)
Protons and Neutrons
22.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
23.
An element with a mass number of 11 and an atomic number of 5 has how many neutrons?
a)
11
b)
5
c)
6
d)
16
24.
Which letter represents a proton?
a)
A
b)
B
c)
C
d)
D
25.
Which letter represents a neutron?
a)
A
b)
B
c)
C
d)
D
26.
Which letter represents an electron?
a)
A
b)
B
c)
C
d)
D
27.
Which letter represents the nucleus?
a)
A
b)
B
c)
D
d)
E
28.
Which subatomic particle has a positive (+) charge?
a)
Neutron
b)
Proton
c)
Electron
29.
Which subatomic particle has a neutral or no charge?
a)
Proton
b)
Electron
c)
Neutron
30.
How did Mendeleev arrange the elements?
a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
31.
The horizontal row on the periodic table is called a
a)
group
b)
family
c)
period
d)
atomic number
32.
The number at the bottom of each square on the periodic table is the ...
a)
atomic number
b)
atomic mass
c)
chemical symbol
d)
element name
33.
The number at the top of each square on the periodic table is the ...
a)
atomic number
b)
atomic mass
c)
Chemical Symbol
d)
Element Name
34.
All of the actinides are ___________.
a)
stable
b)
radioactive
c)
shiny
d)
named after scientists
35.
Most of the elements on the periodic table are classified as _____.
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Periods
36.
This class of elements are sometimes called "semiconductors."
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Groups
37.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
38.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
39.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
40.

Vertical columns of elements (these are also known as a "family") - they also have the same number of valence electrons and are known as ________________.

a)

groups

b)

periods

c)

quadrants

d)

rows

41.
The family in the periodic table that contains the most reactive metals is the_______
a)
Alkaline Earth Metals
b)
Transition Metals 
c)
Alkali Metals
d)
Other Metals
42.

Most noble gases have _______ valence electrons.

a)

1

b)

2

c)

7

d)

8

43.
In what section would Noble Gases be found?
a)
white
b)
yellow
c)
blue
d)
red
44.
All elements found on the left side of the Periodic Table of the Elements have what properties in common?
a)
They conduct heat and electricity 
b)
They are all gases 
c)
They are brittle and dull
d)
They are radioactive
45.

1. The atomic number identifies the number of __________.

a)

protons and electrons

b)

electrons and neutrons

c)

atoms

d)

neutrons and protons

46.

3. The number 16 for the atomic element sulfur is the

a)

ionic number

b)

atomic mass

c)

isotope

d)

atomic number

47.

4. An elements in group 18 are non reactive, stable, and inert because

a)

they have 3 valence electrons and a full outer shell

b)

they have no valence electrons and a full outer shell

c)

they have 8 valence electrons and a full outer shell

48.

5. The group number equals?

a)

The number of energy levels

b)

The number of neutrons

c)

The number of protons

d)

The number of valence electrons

49.

Elements in the same ____________ have similar chemical properties

a)

period

b)

staircase

c)

group

d)

row

50.

Why is group 1 highly reactive?

a)

It has the most energy levels

b)

It has 1 valence electrons

c)

It has the same number of protons

d)

It has the same number of electrons

51.

Which of the following would change the name of the element if one was added or removed from the atom?

a)

neutrons

b)

protons

c)

valence electrons

d)

electrons

52.

The elements Potassium, Vanadium, Manganese and Calcium are examples of

a)

Members of a period

b)

Members of a family

c)

Molecules

d)

Gases

53.

Which element has a mass number greater than nitrogen, but less than neon?

a)

Oxygen

b)

Lithium

c)

Sodium

d)

Helium

54.

Which of the following elements is a metalloid?

a)

Sulfur

b)

Silicon

c)

Iron

d)

Copper

55.

Which of the following elements is malleable?

a)

Iron

b)

Carbon

c)

Hydrogen

d)

Sulfur

56.

What is the mass number of Potassium (K) atom that has 20 neutrons?

a)

18

b)

20

c)

19

d)

39

57.

In an atom, the number of protons is equal to the number of ____________.

a)

energy levels

b)

neurons

c)

electrons

d)

neutrons

58.

The atom that has an atomic mass of 12 has ____________ protons.

a)

6

b)

8

c)

1

d)

4

59.

The periodic table is a chart that organizes the elements based on their atomic properties. Elements in the periodic table are organized according to the periodic law. The periodic law states that chemical and physical properties of elements are periodic functions of their atomic numbers (the number of protons in the nucleus). As the atomic number of elements increases, different elements display similar characteristics at regular intervals.


Periodic law states that elements are arranged _______________________________________________________________.

a)

in alphabetical order.

b)

from largest to smallest.

c)

as periodic functions of their atomic numbers.

d)

there is no rhyme or reason.

60.

In 1869, Dmitri Mendeleev developed the first periodic table, organizing the elements according to atomic weight. When he ordered the elements, he noticed that there were patterns of repeating properties. The modern periodic table sequences elements from left to right by atomic number.


This was the first person to organize a periodic table.

a)

Neils Bohr

b)

Dmitri Mendeleev

c)

Democritus

d)

Ernest Rutherford

61.

It stacks the elements in columns according to the number of valence electrons in an atom of the element. Valence electrons are those in the outermost shell of the atom and the ones that participate in reactions. The number of valence electrons is associated with the element’s reactivity. Elements with the same number of valence electrons behave in a similar way in reactions and so are grouped together in the same column on the periodic table.


What does the amount of valance electrons determine about an element?

a)

Its row in the table.

b)

Its atomic number.

c)

Its atomic mass.

d)

Its reactivity with other elements.

62.

The maximum number of valence electrons an atom can have is eight, with the exception of helium, which can have only two. In each row, or period, of the periodic table, the last element on the right has the maximum number of valence electrons. Its outermost shell is full, and a new period in which the element on the far left has only one valence electron begins in the next row.


How do you determine how many valance electrons an element has?

a)

Count how far over it is from the left in its row.

b)

Count which row it is in.

c)

They all have eight.

d)

You can not determine this from the periodic table.

63.

In the periodic table, similar elements are arranged in vertical columns called groups. Some of the major groups include Group 1: alkali metals; Group 2: alkaline earth metals; Group 17: halogens; and Group 18: noble gases. Elements within each group have similar properties and characteristic behaviors because of their similar numbers of valence electrons.


In what direction are groups arranged in the periodic table?

a)

Side to side

b)

Up and down.

c)

Diagonally

d)

In sections.

64.

Alkali metals have 1 valence electron, making them highly reactive. With the exception of hydrogen, they tend to be very soft metals with low melting points. Examples include sodium and potassium.

Alkaline earth metals have 2 valence electrons and also are highly reactive and have high melting points. Examples include calcium and magnesium.

Halogens have 7 valence electrons and therefore are highly reactive. They tend to form compounds in nature. Examples include chlorine and fluorine.

Noble gases have a complete outer shell with 8 valence electrons, making them nonreactive. They are typically colorless, odorless gases. Examples include helium, neon, and argon.


Which group of elements tend to form compounds in nature?

a)

Alkaline metals

b)

Alkaline Earth metals

c)

Halogens

d)

Noble Gases

65.

Alkali metals have 1 valence electron, making them highly reactive. With the exception of hydrogen, they tend to be very soft metals with low melting points. Examples include sodium and potassium.

Alkaline earth metals have 2 valence electrons and also are highly reactive and have high melting points. Examples include calcium and magnesium.

Halogens have 7 valence electrons and therefore are highly reactive. They tend to form compounds in nature. Examples include chlorine and fluorine.

Noble gases have a complete outer shell with 8 valence electrons, making them nonreactive. They are typically colorless, odorless gases. Examples include helium, neon, and argon.


Which group is highly reactive with high melting points?

a)

Alkaline metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

66.

The periodic table is further arranged into three major regions, including the metals, metalloids, and non-metals. Metals are on the left of the table; they are shiny and flexible, conduct heat and electricity, and participate in ionic reactions. Non-metals are on the far right of the table; they are dull and brittle, are poor conductors, and typically participate in ionic reactions.


Which one is NOT a major region of elements in the periodic table?

a)

Metals

b)

Mettaloids

c)

Non metals

d)

Gases

67.

Carbon and silicon, however, are examples of non-metals that participate in covalent reactions. Metalloids are located in a zig-zagging line between the two other regions. Metalloids are solid semi-conductors. In contrast to metals and non-metals, metalloids participate in covalent reactions.


Where would you look on the table to find the mettaloids?

a)

In a zigzag line on the right.

b)

In column 17

c)

On the bottom

d)

On the top

68.

The elements in groups 3-12 are called the transition metals. These are similar to the metals in that they are flexible and good conductors but different in that they have unique valence electron structure. They typically form coordinate complexes in which one atom is surrounded by several more in a large complex. Iron, gold, and copper are examples of transition metals.


Which group are the transition metals most like?

a)

Metals, they are flexible and good conductors.

b)

Non metals, they a unique valence electron structure.

c)

Noble gases, they don't want to bond with anything else.

d)

They are like both metals and non metals in some ways.

69.

The nucleus of an atom contains which of the following subatomic particles: (Select two)

a)

protons

b)

Neutrons

c)

Electrons

d)

Shells

70.

Hydrogen has an atomic number of 1. How many electrons does hydrogen have?

a)

1

b)

2

c)

4

d)

0

71.

The atomic number will tell me... (select three)

a)

Number of Protons

b)

Number of Electrons

c)

Number of Neutrons

d)

What element is it

72.

Which are of the following are subatomic particles. Select three:

a)

Protons

b)

Neutrons

c)

Electrons

d)

Nucleus

73.

Silicon has an atomic number of 14 and an atomic mass of 28. How many neutrons does it have?

a)

14

b)

28

c)

2

d)

10

74.

Which of the following are properties of a metal: (you should select more than one)

a)

Good conductor of heat and electricity

b)

Brittle (break easily)

c)

Malleable (able to bend without breaking)

d)

Luster (shiny)

e)

Dull

75.

This element is found in group 2, period 3:

a)

Li

b)

Mg

c)

Be

d)

B

76.

Valence electrons are:

a)

Just the electrons on the last energy level (outer shell)

b)

All the electrons in the atom

77.

Which diagram would you draw if you wanted to represent just the valence electrons?

a)

Electron Configuration

b)

Lewis Dot

c)

Bohr Model

78.

What best describes the difference between the bohr model and the lewis dot?

a)

The bohr model diagram represents all the subatomic particles, while the lewis dot diagram only shows the symbol and the valence electrons.

b)

The lewis dot shows all the electrons and the bohr model only shows the electrons in the last shell

c)

The lewis dot shows the number of neutrons and the bohr model only shows the electrons

79.

What is the charge of a proton?

a)

Positive

b)

Negative

c)

No charge, Neutral

80.

What is the charge of an electron?

a)

Postive

b)

Negative

c)

No Charge

81.

Which of the following is the electron configuration for Magnesium, Mg? (Atomic number 12)

a)

2-4-4

b)

2-8-2

c)

2-8

d)

2-4-6

82.

This diagram represents the atom of what element?

a)

Kr (Krypton)

b)

Cd (Cadmium)

c)

Se (Selenium)

d)

Ca (Calcium)

83.

A student drew a lewis dot structure with 7 valence electrons. Which of the following elements might have the student drawn?

a)

Cl (Chlorine)

b)

Ne (Neon)

c)

N (Nitrogen)

d)

Li (Lithium)

84.
Sodium (Na) and potassium (K) are in the same group on the periodic table. Based on their locations, which statement about sodium and potassium is true?
a)
Sodium is less electronegative than potassium. 
b)
Sodium has fewer energy levels than potassium. 
c)
Sodium has a larger ionic radius than potassium. 
d)
Sodium has lower ionization energy than potassium. 
85.
Which of these elements has the greatest atomic radius? 
a)
H
b)
N
c)
Cl
d)
Cs
86.
The Periodic Table of the Elements is useful for revealing patterns and trends in the elements. Which statement accurately describes a pattern in the size of atomic radii in the Periodic Table of the Elements?
a)
Atomic radii decrease from left to right across a period and decrease from top to bottom in a group.
b)
Atomic radii increase from left to right across a period and increase from top to bottom in a group.
c)
Atomic radii decrease from left to right across a period and increase from top to bottom in a group.
d)
Atomic radii increase from left to right across a period and decrease from top to bottom in a group.
87.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
88.
Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the greatest ionization energy and electronegativity?
a)
fluorine
b)
chlorine 
c)
bromine 
d)
iodine 
89.
The ionization potential of an element is the amount of energy required to remove an electron from an isolated atom or molecule. According to the periodic table, which of the following indicates the correct decreasing order of ionization energy?
a)
Li > Na > K > Cs
b)
Na > K > Li > Cs
c)
Li > K > Na > Cs 
d)
Cs > K > Na > Li 
90.
Which of these elements has an electron structure most similar to that of element X?
a)
1
b)
2
c)
3
d)
4
91.
Based on their locations in the periodic table, which element has chemical properties most similar to those of calcium, Ca?
a)
beryllium, Be
b)
potassium, K
c)
titanium, Ti
d)
yttrium, Y
92.
The number of valence electrons in an element affects the reactivity of that element. Which element listed has the fewest valence electrons?
a)
beryllium (Be)
b)
sodium (Na) 
c)
oxygen (O) 
d)
neon (Ne)
93.
According to the Periodic Table of the Elements, which set of elements has similar properties?
a)
H, C, I
b)
He, H, Al
c)
He, Ne, Ar
d)
Na, Ca, Al
94.
What is the family name of this group of elements? 
a)
Alkali metals 
b)
Halogens 
c)
Noble Gases 
d)
Alkali Earth Metals 
95.
Which element has 2 valence electrons? 
a)
cesium (Cs) 
b)
magnesium (Mg)
c)
boron (B)
d)
argon (Ar) 
96.
How many Valance electrons does Iodine Have?
a)
6
b)
16
c)
7
d)
17
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.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
99.
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. 
100.
Metals have the largest - 
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
101.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
102.
As you move down the periodic table atoms get 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 neutrons
103.
Describe an Electron Cloud?
a)
the mist outside of an atom
b)
home of the protons
c)
where electrons are located
d)
nucleus
104.
The subatomic particle that determines the identity of an element.
a)
neutron
b)
proton
c)
electron
d)
outer shell
105.
What is the atomic number of the atom pictured? 
a)
11
b)
12
c)
22
d)
23
106.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
107.
Which of the following is a substance that can not be broken down into a simpler substance?
a)
Isotope
b)
Element
c)
Compound
d)
Atomic Number
108.
What is at the center of every atom?
a)
An electron
b)
A compound
c)
A molecule
d)
A nucleus
109.
In an atom, what is the number of protons equal to?
a)
The number of electrons.
b)
The number of neutrons.
c)
The number of molecules.
d)
The number of nuclei.
110.
The negatively charged particles of an atom are the ______.
a)
electrons
b)
protons
c)
neutrons
d)
protons & neutrons
111.
What number indicates an electron?
a)
1
b)
2
c)
3
d)
4
112.
What number indicates the nucleus?
a)
1
b)
2
c)
3
d)
4
113.

Which statement correctly describes the location and charge of the neutrons in an atom?

a)

The neutrons are inside the nucleus and have a positive charge.

b)

The neutrons are outside the nucleus and have a neutral charge.

c)

The neutrons are outside the nucleus and have a negative charge.

d)

The neutrons are inside the nucleus and have a neutral charge.

114.

Mass minus Atomic Number Equals (M-A=?)

a)

Neutrons

b)

Protons

c)

Nucleus

d)

Atom

115.

Atomic number equals ______________ and _______________

a)

Neutrons

b)

Protons

c)

Electrons

d)

Elements

116.

How many neutrons does this element have?

a)

1

b)

2

c)

3

d)

4

117.

What goes in place of the question marks?

a)

Element name

b)

Atomic Mass

c)

Atomic Number

d)

Electrons

118.

What goes in place of the question marks?

a)

Neutrons

b)

Electron Cloud

c)

Atomic Number

d)

None of the above

119.

APE MAN stands for

a)

Atomic Number=Protons=Electrons

Atomic Mass-Atomic Number=Neutrons

b)

Atomic Mass=Pictures=Eating

Mass- Atomic Number= Element Name

c)

Atomic Number= Periodic Table=Elements

Atomic Mass-Atoms=Notes

120.

Where do the electrons hangout?

a)

Electron Cloud

b)

Nucleus

c)

Atom Cloud

121.

How many subatomic particles are there in an Atom?

a)

1

b)

2

c)

3

d)

Infinite

122.

What is Group 18 referred as?

a)

Halogens

b)

Alkaline

c)

Alkali

d)

Noble Gases

123.

What Element is H?

a)

Helium

b)

Hydrogen

c)

Hectogen

d)

Not enough information

124.

Where will you find electrons in an atom?

a)

Nucleus

b)

Moving around the nucleus

c)

Directly next to a proton

d)

Atoms don't have electrons, only protons and neutrons

125.

Which particle tells you which element you are?

a)

Proton

b)

Neutron

c)

Quark

d)

Electron

126.

What is an element called if it has more or less neutrons than the stable version of the element?

a)

Isotope

b)

Ion

c)

Negative

d)

Positive

127.

Which particles contribute to the mass of an atom?

a)

How much space they take up

b)

Protons and Neutrons

c)

Electrons and Quarks

d)

Protons and Electrons

128.

How many protons are in this atom?

a)

28

b)

14

c)

29

d)

42

129.

How many neutrons are in this element?

a)

28

b)

14

c)

29

d)

42

130.

How many protons are in Boron?

a)

2

b)

5

c)

7

d)

10.8

131.

True or False: Neutrons are negatively charged.

a)

True

b)

False

132.

When building a Bohr Model, what is the MAXIMUM number of electrons you can have on the FIRST shell?

a)

1

b)

2

c)

8

d)

18

133.

What element is in Period 2 Group 4?

a)

Calcium

b)

Carbon

c)

Titanium

d)

Doesn't Exist

134.

Which group on the periodic table is the Most reactive?

a)

18

b)

Halogens

c)

17

d)

Noble gases

135.

What is the element Symbol for Aluminum?

a)

A

b)

AL

c)

Al

d)

Am

136.

When building a Bohr Model, what is the MAXIMUM number of electrons you can have on the SECOND shell?

a)

1

b)

2

c)

8

d)

18

137.

What is the atomic mass for Carbon? (Rounded)

a)

15

b)

13

c)

16

d)

12

138.

How many electrons are in Potassium?

a)

15

b)

19

c)

39.10

d)

30.97

139.

Which of the following elements are in Period 4?

a)

Titanium

b)

Beryllium

c)

Argon

d)

Calcium

140.

Why is the Periodic Table shaped the way it is?

a)

To make room for elements we haven't discovered

b)

Because it wouldn't work any other way

c)

This is just one layout that the scientific community likes

d)

Because it looks like an upside-down table

141.

How are the elements in the modern periodic table arranged?

a)

atomic mass

b)

chemical symbol

c)

element's name

d)

atomic number

142.

All the matter is made up of the same atom. Which sentence correctly describes atoms?

a)

All substances are made of the same atom.

b)

An atom is the smallest particle of the nucleus.

c)

An atom is the smallest particle of an element.

d)

An atom is a substance that has been cut in half.

143.

Use your periodic table. What is the atomic number for iron?

a)

26

b)

56

144.

How many electrons does a sodium atom contain?

a)

23

b)

11

145.

What subatomic particle has a positive charge?

a)

electron

b)

neutron

c)

proton

146.

Group 18 elements are called the ______ ______.

a)

alkali metals

b)

alkaline earth metals

c)

noble gases

d)

transition metals

147.

Neutrons are found in the nucleus of an atom and have a (a)   charge.

148.

Use your periodic table. The element neon has

a)

10 protons, 20 neutrons, 12 electrons

b)

15 protons, 15 neutrons, 15 electrons

c)

0 protons, 0 neutrons, 0 electrons

d)

10 protons, 10 neutrons, 10 electrons

149.

The columns of the periodic table are called _____ while the rows are called _____.

a)

groups/families, periods

b)

periods, groups/families

150.

The atomic number of an atom tells the number of (a)   in the nucleus.

151.

The outermost electrons are called ______ electrons.

a)

nothing

b)

valence

c)

electron cloud

d)

energy levels

152.

Metals have a shiny luster while nonmetals have a _____ luster.

a)

shiny

b)

dull

c)

neither shiny or dull

153.

How many valence electrons does group 2 contain?

(a)  

154.

Lanthanides and Actinides are part of groups 3-12 which are called ______ metals.

a)

transition

b)

alkali

c)

alkaline earth

155.

Use your periodic table. What element is in group 10, period 4?

a)

copper

b)

nickel

c)

cobalt

d)

palladium

156.

Charles needs a very lightweight metal. Use the periodic table to determine which he would choose.

a)

silicon

b)

magnesium

c)

iodine

d)

tungsten

157.

Use your periodic table. What is the atomic mass of boron?

(a)  

158.

Which of these does the number of electrons in the outer level (valence electrons) indicate about the element?

a)

its reactivity

b)

its atomic number

c)

its atomic mass

d)

its symbol

159.

Look at your periodic table of elements for cobalt (27) and nickel (28). What is the biggest difference between an atom of cobalt (Co) and an atom of nickel (Ni) as show in the periodic table?

a)

An atom of nickel has more protons.

b)

An atom of cobalt has more electrons.

c)

An atom of cobalt has more neutrons.

d)

An atom of nickel has a higher value for atomic mass.

160.

What are the elements in group 1 (the far left) of the periodic table called?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

161.

What are the elements in group 2 of the periodic table called?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

162.

What are the elements in group 18 (the far right) of the periodic table called?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

163.

What are the elements in group 17 of the periodic table called?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

164.

What are the elements in groups 3-12 of the periodic table called?

a)

Transition metals

b)

Non-metals

c)

Metalloids

d)

Metals

165.

What are the elements found along the "staircase" called? They have properties of both metals and non-metals.

a)

Metalloids

b)

Non-metals

c)

Transition metals

d)

Metals

166.

Hydrogen is a:

a)

Alkali metal

b)

Metalloid

c)

Non-metal

d)

Noble gas

167.

The Russian scientist who created one of the first periodic tables by using atomic mass was:

a)

Bohr

b)

Rutherford

c)

Mendeleev

d)

Thomson

168.

The subatomic particles that are located the farthest from the nucleus are:

a)

Valence electrons

b)

Valence protons

c)

Periodic electrons

d)

Periodic protons

169.

The number of electron shells an atom has is equal to the element's:

a)

Period number

b)

Group number

c)

Valence number

d)

Atomic number

170.

The model of an atom that shows electrons in circular orbits around the nucleus is called the:

a)

Bohr Model

b)

Lewis Dot Structure

c)

Rutherford Model

d)

Thomson Model

171.

The model of an atom that uses dots surrounding the atomic symbol to represent valence electrons is called the:

a)

Bohr Model

b)

Lewis Dot Structure

c)

Rutherford Model

d)

Thomson Model

172.
These determine the reactivity of an element...
a)
Valence electrons
b)
Valence Protons
c)
Valence Neutrons
d)
Valence Quark
173.
How many protons are in Cadmium?
a)
112.411
b)
170
c)
64
d)
48
174.
How many neutrons does Argon have in it's nucleus?
a)
39.948
b)
58
c)
22
d)
18
175.
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)
176.
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
177.

What is one difference between aluminum (Group 13) and magnesium's (Group 2) structure?

a)

Aluminum has more protons and fewer neutrons than magnesium.

b)

Magnesium has one more proton than aluminum.

c)

Magnesium's atomic mass is larger than aluminum's atomic mass.

d)

Magnesium has one less proton than aluminum.

178.
What period and group is Silver (Ag)? 
a)
Period 2, Group 1
b)
Period 3, Group 16
c)
Period 5, Group 11
d)
Period 2, 14
179.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
180.
The period for Bromine is ___________.
a)
3
b)
2
c)
4
181.
How many Valance electrons does Iodine Have?
a)
6
b)
16
c)
7
d)
17
182.
The elements in a column of the periodic table...
a)
have similar atomic numbers
b)
start with the same letter
c)
have similar properties
d)
are not related in any way
183.
Which of the following has six valence electrons?
a)
Sodium
b)
Iodine
c)
Oxygen
d)
Neon
184.
What is the atomic mass of "F"
a)
9
b)
18
c)
17
d)
19
185.

Which statement is accurate regarding subatomic particles?

a)

electrons are the heaviest particle, with a positive charge

b)

protons and electrons are equal in mass with positive charges

c)

electrons are neutral with the least mass

d)

protons have a positive charge with a mass of 1 amu and neutrons are neutral with the same mass as a proton

186.

Which atom has a nucleus that contains 13 protons and 14 neutrons?

a)

Mg

b)

Be

c)

Al

d)

N

187.

The most reactive metals are the

a)

alkali metals

b)

alkali earth metals

c)

transition metals

d)

metalloids

188.

The elements with largest atomic radii are found

a)

across the top of the periodic table

b)

on the far right side of the periodic table

c)

the bottom left corner

d)

the top right corner

189.

As you move up and to the right on the periodic table

a)

atomic radii increase

b)

ionization energy and electronegativity increase

c)

elements with metallic properties are found

d)

transition metals corrode

190.

Which of the following is NOT true regarding families (groups) on the periodic table?

a)

they have similar characteristics

b)

they have the same number of valence electrons

c)

the atomic radius increases as you go down

d)

groups are identical to periods on the periodic table

191.
What is the mass number of this atom?
a)
1
b)
3
c)
4
d)
7
192.

On the periodic table, Periods are

a)

Horizontal rows

b)

Vertical columns

193.
How many "valance electrons" are in chlorine?
a)
7
b)
2
c)
17
d)
8
194.
Carbon-12, Carbon-13, and Carbon-14 are...
a)
ions
b)
isotopes
c)
electronegative
d)
radioactive
195.
Nitrogen has 5 valence electrons
a)
True
b)
False, it has 7
c)
False, it has 14
d)
False, it has 7.01
196.
An isotope has...
a)
the same number of protons but different number of electrons
b)
same number of protons but different number of neutrons
c)
same number of electrons and neutrons
d)
same number of electrons, protons, and neutrons
197.
Elements that are gases, brittle, and not conductive are
a)
Metals
b)
Metalloids
c)
Transition Metals
d)
Non-metals
198.
Not non-metals or metals but somewhere in between
a)
noble gases
b)
isotopes
c)
metalloids
d)
ions
199.
Is this Lewis Dot Structure correct
a)
Yes
b)
No, chlorine has 6 valence
c)
No, chlorine has 8 valence
d)
No, chlorine has 17 electrons
200.
What is titanium's atomic mass?
a)
47.867
b)
22
c)
26
d)
49
201.
The atomic mass of Boron is 10.81, which means Boron has..
a)
5 electrons and 6 protons, each weigh 1 amu
b)
5 neutrons and 6 electrons, each weigh 1 amu
c)
6 neutrons and 5 protons, each weigh 1 amu
d)
10.81 protons each weighing around 1 amu
202.
Who arranged the first periodic table.
a)
Mosely
b)
Einstein
c)
Mendeleev
d)
Bohr
203.
What was Dmitri Mendeleev's greatest contribution to the history of the periodic table?
a)
He arranged all of the known elements by their atomic number
b)
He realised that there was a pattern of reactivity which repeated every 8 elements
c)
He predicted the existence (and properties) of new elements
d)
He identified the "law of triads" which became the groups
204.
Mendeleev classified elements based on not only atomic mass but what else?                                                   
a)
reactivity
b)
boiling points
c)
physical properties only 
d)
 chemical & physical properties
205.
Why were there blank spaces left in Mendeleev's periodic table?                                              
a)
He didn't know what to put there.
b)
 Undiscovered elements not yet known.
c)
Multiple elements could have fit
d)
He forgot to add the elements in.
206.

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

207.

As you move from left to right on the periodic table, the number of valence electrons.......

a)

Increases

b)

Decreases

c)

Remains the same

208.

As you move down a group on the periodic table, the number of valence electrons....

a)

Increases

b)

Decreases

c)

Remains the same

209.

Which of the following is the term for a substance in which all the atoms have the same number of protons

a)

a compound

b)

An element

c)

a molecule

d)

a solid

e)

a gas

210.
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. 
211.
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
212.

Inert gases, non-reactive, belong to this family

a)

Alkali family

b)

Carbon family

c)

Noble gas family

d)

Halogen family

213.

As electronegativity increases, atoms from left to right in a period on the periodic table __________ in atomic radius.

a)

Increase

b)

Decrease

c)

Stays the same

d)

Fluctuates

214.

An atom with high ionization energy has 7 valence electrons, when this atom gains an electron, it becomes a __________ ion.

a)

Positive

b)

Negative

c)

Neutral

d)

Covalent

215.

When two nonmetals share electrons equally due to their similar electronegativities, they form a(n) _________ bond

a)

Ionic

b)

Covalent

c)

Polar covalent

d)

Hydrogen

216.

_________ give away electrons to become positive ions and __________ steal electrons to become negative ions.

a)

Metals, metals

b)

Nonmetals, nonmetals

c)

Nonmetals, metals

d)

Metals, nonmetals

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