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Classifying Matter Review Two

Total questions: 84

Worksheet time: 21hrs 0mins

Name
Class
Date
1.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
2.
An element's identity is determined by the number of
a)
electrons.
b)
protons.
c)
neutrons.
d)
valence.
3.
The atomic number of an element tells the number of _____ in the nucleus of an atom of that element.
a)
protons
b)
neutrons
c)
electrons
d)
isotopes
4.
Most of the mass of an atom is found it its _____.
a)
electron cloud
b)
nucleus
c)
atomic number
d)
empty space
5.
An element is made up of only one kind of _____.
a)
isotope
b)
plastic
c)
atom
d)
metal
6.
What subatomic particles are located in the electron cloud?
a)
quarks
b)
protons
c)
electrons
d)
neutrons
7.
Which subatomic particle has a negative charge in the atom?
a)
proton
b)
neutron
c)
electron
d)
quark
8.
Which is an electron?
a)
A
b)
B
c)
C
9.
Which is a proton?
a)
A
b)
B
c)
C
10.
Which item on this element square is the chemical symbol?
a)
Copper
b)
29
c)
Cu
d)
63.546
11.
Which item on this element square represents the atomic number?
a)
13
b)
Al
c)
Aluminum
d)
26.981538
12.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
13.
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
14.
What are subatomic particles? 
a)
the nucleus 
b)
electron cloud
c)
positive charge
d)
electrons, protons, and neutrons
15.

How do you find the number of neutrons in an atom?

a)

Atomic Number

b)

Atomic Mass

c)

Atomic Mass - Atomic Number

d)

Atomic Number + Atomic Mass

16.

a grouping of elements based on similar properties, arranged by columns in the periodic table; also known as a group

a)

family

b)

period

c)

row

d)

isotope

17.

a row on the Periodic Table of Elements

a)

family

b)

period

c)

row

d)

isotope

18.

one of several forms of a single element, which contains the same number of protons, but different numbers of neutrons

a)

isotope

b)

ion

c)

orbital

d)

nucleus

19.

What are valence electrons?

a)

Any of an atom's electrons

b)

Electrons located on the first energy level

c)

Electrons not attached to any atom

d)

electrons located on the outer energy level

20.

What category is silicon (Si) a part of?

a)

Metal

b)

Nonmetal

c)

Metalloid

d)

Halogens

21.

What is group name of the most reactive metals?

a)

Noble gases

b)

Halogens

c)

Alkali metals

d)

Alkaline earth metals

22.

Why are halogens so reactive?

a)

They want to get rid of their only valance electron

b)

They only need one more electron

c)

They are non reactive, they have a full shell

23.
Name group 1A on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
noble gases
d)
halogens
24.
Name group 2A on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
d)
transition metals
25.
Name group 8A on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
transition metals
d)
noble gases
26.
Name groups 3B - 12B on the periodic table.
a)
noble gases
b)
halogens
c)
metalloids
d)
transition metals
27.
Name group 7A on the periodic table.
a)
transition metals
b)
metalloids
c)
halogens
d)
alkali metals
28.
Which group has the most reactive nonmetals?
a)
alkali metals
b)
noble gases
c)
metalloids
d)
halogens
29.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
30.
Where are the nonmetals located on the periodic table?
a)
top left corner
b)
bottom left corner
c)
top right corner
d)
bottom left corner
31.
The Lanthanide elements are known as the:
a)
Common earth metals
b)
Alkaline earth metals
c)
Rare earth metals
d)
Heavy earth metals
32.
Which statement is true about the carbon family?
a)
They are all non-metals.
b)
They all have four valence electrons.
c)
They are all metals.
d)
They do not react with other elements.
33.

These are found on the Periodic Table.

a)

Compounds

b)

Elements

c)

Mixtures

34.

Which elements have properties in common?

a)

elements in a group

b)

elements in a period

35.

Which element in Period 2 has the greatest atomic radius?

a)

Be

b)

C

c)

Na

d)

Li

36.

Which of the group 13 elements is the largest?

a)

B

b)

Tl

c)

Fr

d)

Ga

37.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

38.

Of the halogens, which has the smallest electronegativity?

a)

F

b)

Cl

c)

At

d)

Ne

39.

Which of the period 3 elements has the largest electronegativity?

a)

Ar

b)

Cl

c)

Na

d)

F

40.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
41.
Which has the greater EN: 
N or C?
a)
C
b)
N
42.
Which has the greater EN: 
H or F?
a)
H
b)
F
43.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
44.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
45.
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)
46.
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
47.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
48.
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 nuetrons
49.
As you move across the periodic table atoms tend 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.
50.
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.
51.
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. 
52.
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
53.
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.
54.
1.  What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
55.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
56.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
57.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
58.
How many total electrons can the f orbitals in a sublevel hold?
a)
2
b)
14
c)
6
d)
10
59.

How many orbitals does an s sublevel have?

a)

1

b)

3

c)

5

d)

7

60.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
61.
How many neutrons would Fe-56 have?
a)
56
b)
26
c)
30
d)
33
62.
How many protons does P-30 have?
a)
30
b)
16
c)
12
d)
15
63.
If an atom of nickel has a charge of +3, how many electrons does the atom have?
a)
28
b)
25
c)
26
d)
31
64.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
65.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
66.
An element is defined by its number of 
a)
protons
b)
electrons
c)
neutrons
d)
protons + electrons
67.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

68.

What does the mass number of an element represent?

a)

The number of protons in an atom

b)

the number of neutrons in an atom

c)

the number of electrons in an atom

d)

the number of protons and neutrons in an atom

69.

What charge does an atom have when it GAINS electrons?

a)

Positive

b)

Negative

c)

Neutral

70.
Which of the following could have 14 neutrons?
a)
Al-27
b)
Si-29
c)
Mg-25
d)
Na-22
71.
In a correctly written symbol what would be located in the "A" position?
a)
number of neutrons
b)
atomic number
c)
number of electrons 
d)
mass number
72.
How many neutrons does a Calcium 48 isotope have?
a)
16
b)
20
c)
28
d)
12
73.
In a stable atom the amount of electrons is electron is equal to
a)
neutrons
b)
protons
c)
atomic mass
d)
neutrons + protons
74.
The first orbital can hold a maximum of how many electrons?
a)
2
b)
3
c)
8
d)
6
75.
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
76.
What property did Menedleev use to organize his first periodic table?
a)
atomic number
b)
atomic mass
c)
alphabetical order
d)
chemical properties
77.
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.
78.
Moseley discovered that the ________ was the most fundamental property needed for organization.                                                 
a)
atomic mass
b)
mass number
c)
atomic number
d)
number of protons
79.

The "Law of Octaves" stated that

a)

The properties of the elements repeated every eighth element when arranged by their atomic mass

b)

Elements could be classified in groups of three based on their mass and properties

c)

The properties of the elements repeated of a regular basis when arranged by their atomic number

d)

doubling the frequency of a tone raises its pitch by an octave

80.

The "Law of Octaves" was the brainchild of

a)

Glenn Seaborg

b)

Lothar Meyer

c)

Johann Dobereiner

d)

John Newlands

81.

Where are the s sublevels located based on the periodic trend?

a)

groups 1A and 2A (plus helium)

b)

transition metals

c)

inner transition metals

d)

groups 3A to 8A (minus helium)

82.

Where are the p sublevels located based on the periodic trend?

a)

groups 1A and 2A (plus helium)

b)

transition metals

c)

inner transition metals

d)

groups 3A to 8A (minus helium)

83.

Where are the d sublevels located based on the periodic trend?

a)

groups 1A and 2A (plus helium)

b)

transition metals

c)

inner transition metals

d)

groups 3A to 8A (minus helium)

84.

Where are the f sublevels located based on the periodic trend?

a)

groups 1A and 2A (plus helium)

b)

transition metals

c)

inner transition metals

d)

groups 3A to 8A (minus helium)

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