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Periodic Trends HW

Total questions: 40

Worksheet time: 43mins

Name
Class
Date
1.
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
2.
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.
3.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
4.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
5.
Order the following in increasing atomic radii: 
Ra, Be, Ca, Rb, H
a)
Ra, Be, Rb, H, Ca
b)
Rb, H, Ca, Be, Ra
c)
Ra, Rb, Ca, Be, H
d)
H, Be, Ca, Rb, Ra
6.
The more protons there are, the  ____ .
a)
Weaker the pull
b)
Smaller the electrons
c)
Stronger the pull
d)
The bigger the electrons
7.
Which one has the largest radius?
a)
Lithium (Li, atomic #3)
b)
Boron (B, atomic #5)
c)
Neon (Ne, atomic #10)
d)
Nitrogen (N, atomic #7)
8.

What is the atomic radius?

a)

The distance from the nucleus to the outer boundary of an atom

b)

The distance from one side of an atom to the other side

c)

The distance around the atom

d)

The distance between atoms in the gas phase

e)

The distance between atoms in the solid phase

9.

Which of the following elements would be the largest: copper, zinc, silver or cadmium?

a)

copper

b)

zinc

c)

silver

d)

cadmium

e)

cannot be determined

10.

Why is iodine larger than bromine?

a)

iodine has a greater number of electrons than bromine

b)

iodine has a greater number of protons than bromine

c)

iodine has more occupied energy levels and greater shielding than bromine

d)

iodine has more neutrons than bromine

e)

iodine has more valence electrons than bromine

11.

Which species has the larger radius?

a)

Cl

b)

Cl-

12.

Which species has the larger radius?

a)

Na

b)

Na+

13.
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 
14.

Which of the following ions is larger

a)

Ca2+

b)

Mg2+

15.
Put these in increasing order:
F, N, B
a)
B < N < F
b)
B < F < N
c)
N < F < B
d)
F < N < B
16.
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. 
17.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
18.
Elements closer to the noble gases have stronger attraction for electrons.
a)
True
b)
False
19.
What elements have zero electronegativity?
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
20.

Which element has a higher electronegativity value?

a)

Niobium

b)

Tin

c)

Cadmium

d)

Iodine

21.

Electronegativity trends are the same as:

a)

Atomic radius trends

b)

Ionization energy trends

c)

Both of these

d)

None of these

22.

What does electronegativity do as you go across a period?

a)

decrease

b)

no pattern

c)

stay the same

d)

increase

23.

Which is the correct order of electronegativity from lowest to highest?

a)

Zinc, Nickel, Iron, Scandium

b)

Iron, Nickel, Zinc, Scandium

c)

Scandium, Iron, Nickel, Zinc

d)

Scandium, Iron, Zinc, Nickel

24.
What is ionization energy?
a)
Energy needed to destroy an atom
b)
Energy required to remove an electron
c)
Energy needed to split an electron
d)
Energy required to add an electron
25.

Which element has the greater ionization energy?

a)

Magnesium (Mg)

b)

Phosphorus (P)

26.
List the following in order of weakest to strongest ionization energy.
P, Cs, Co, Sr
a)
P, Co, Sr, Cs
b)
Cs, Sr, Co, P
c)
Sr, Cs, Co, P
d)
P, Co, Cs, Sr
27.

Who developed the Periodic Table?

a)

Mendeleev, who was a chemist and teacher

b)

Pavlov, who was a teacher and physchologist

c)

Ladahoff, who was a teacher and biologist

28.
The tendency of an atom to attract electrons and acquire a negative charge
a)
electronegativity
b)
charge
c)
bonding ability
d)
electron configuration
29.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

30.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
31.
Which of these is a property of metals?
a)
It's malleable
b)
It can't conduct electricity
c)
They are used in food
d)
It's very brittle
32.

What is a cation's charge?

a)

positive

b)

negative

c)

neutral

d)

depends on the element

33.

What is an anion's charge?

a)

positive

b)

negative

c)

neutral

d)

depends on the element's charge

34.

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

a)

groups

b)

towers

c)

periods

d)

atomic numbers

35.

When atom gains an electron, the size will

a)

increase

b)

decrease

c)

have no change

d)

smaller

36.
Name group 2 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
d)
transition metals
37.
Name groups 3 - 12 on the periodic table.
a)
noble gases
b)
halogens
c)
metalloids
d)
transition metals
38.
How many valence electrons are found in atoms of group 1?
a)
7
b)
6
c)
4
d)
1
39.
How many valence electrons are in an atom of Se?
a)
2
b)
8
c)
6
d)
5
40.
Put the following in order of increasing ionization energy:Neon, Lithium, Carbon
a)
Lithium, Carbon, Neon
b)
Carbon, Lithium, Neon
c)
Neon, Carbon, Lithium
d)
Lithium, Neon, Carbon

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