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Periodicity

Total questions: 15

Worksheet time: 18mins

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.
Which is larger... P or P3- ?
a)
P3- because it gains an energy level
b)
P3- due to extra electron repulsion
c)
P because it loses an energy level
d)
P because of extra electron repulsion
3.

Why does ionization energy decrease going down a group?

a)

Adding more energy levels takes the electron further from the nucleus so it is easier to remove

b)

There are more valence electrons in the outer shell so the ve- is easier to remove

c)

There are more protons in the nucleus so the ve- is easier to remove

d)

There are less protons in the nucleus so the ve- is easier to remove

4.
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 shells

d)
The atoms have more nuetrons
5.
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. 
6.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

7.
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
8.

What makes a valence electron more attracted to the nucleus?

a)

less distance between the nucleus and having less protons

b)

less distance between the nucleus and having more protons

c)

more distance between the nucleus and having less protons

d)

more distance between the nucleus and having more protons

e)

less distance and having more valence electrons

9.

The higher the ionization energy...

a)

the more attracted the valence electron is to the nucleus so it is harder to remove

b)

the less attracted the valence electron is to the nucleus so it is easier to remove

c)

the more attracted the valence electron is to another electron, so it is harder to remove

d)

the more repelled a valence electron is to another electron, so it is easier to remove

10.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
11.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
12.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
13.

The correct electron configuration for Chlorine is

a)

1s22s22p5

b)

1s22s22p63s2

c)

1s22s22p63s23p4

d)

1s22s22p63s23p5

14.

What is the mean of the "halogens"?

a)

acid former

b)

salt former

c)

alkali former

d)

non metal former

15.

Which of the "Halogens" is found in liquid state at room temperature?

a)

Flourine

b)

Astatine

c)

Iodine

d)

Bromine

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