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Periodic Table and e- configuration

Total questions: 26

Worksheet time: 52mins

Name
Class
Date
1.

Which element has seven valence electrons? (Belongs to the Halogen family)

a)

Chlorine (Cl)

b)

Lead (Pb)

c)

Argon (Ar)

d)

Sulfur (S)

2.

Which of the following react violently with water, producing hydrogen gas?

a)

Alkali metals

b)

Noble gases

c)

Halogens

d)

Transition metals

3.

Which of the following properties can be expected for halogens such as fluorine (F) and chlorine (Cl) based on their valence e-? (SELECT TWO CORRECT ANSWERS).

a)

Gain one e- during chemical reaction

b)

React readily with Group 1 metals

c)

Same number of electron shells

d)

Similar reaction rates

4.

The Halogen group has an oxidation number of -1. Why?

a)

The Halogen group will gain one electron, therefore have an oxidation number of -1.

b)

The Halogen group will lose one electron, therefore have an oxidation number of -1.

c)

The Halogen group will lose seven electrons, therefore have an oxidation number of -1.

5.

Dimitri Mendeleev is most famous for-

a)

organizing elements by atomic mass

b)

arranging the Periodic Table by chemical properties

c)

calculating atomic number of many elements

d)

discovering many new elements, such as oxygen

6.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
7.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
8.

Metals (like Na) typically _____ electrons in the formation of ionic bonds.

a)

Gain

b)

Lose

c)

Keep the same

9.

Which list of elements from Group 2 on the Periodic Table is arranged in order of increasing atomic radius? (Smallest to Largest)

a)

Be, Mg, Ca

b)

Ca, Mg, Be

c)

Ba, Ra, Sr

10.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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. 
11.
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
12.
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
13.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
14.

Which electron configuration belongs to a Sulfur?

a)

1s2 2s2 2p6 3s2 3p4

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p7

d)

1s2 2s2 2p6 3p7

15.

Put the following in order of increasing ionization energy:Neon (Ne), Lithium (Li), Carbon (C)

a)
Lithium, Carbon, Neon
b)
Carbon, Lithium, Neon
c)
Neon, Carbon, Lithium
d)
Lithium, Neon, Carbon
16.

Put these in increasing order of electronegativity:
C, H, and O

a)
H < C < O
b)
H < O < C
c)
O < C < H
d)
C < H < O
17.

Covalent bonds occur when electrons are _______________________.

a)

Transferred

b)

Shared

c)

Lost

d)

Gained

18.

What is the total electrons that is shown the given orbital diagram?

a)

6

b)

7

c)

8

d)

9

19.

Which element is represented in the given orbital diagram?

a)

Carbon (C)

b)

Hydrogen (H)

c)

Nitrogen (N)

d)

Oxygen (O)

20.

Subshell are represented by

a)

a box

b)

letters s, p, d, and f

c)

a number

d)

none the choices.

21.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
22.

states that electrons that is sharing an orbital have opposite spins

a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
23.

electrons will occupy an empty orbital when it is available in that subshell

a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
24.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Nitrogen (N)
b)
Lithium (Li)
c)
Antimony (Sb)
d)
Germanium (Ge)
25.

Elements of the same ______________ have the same number of valence electrons, which determines the elements chemical properties.

a)

Period

b)

Row

c)

Group

26.

Atoms are most stable when their outermost shell is full. If their outermost shell is not full, _______ to have a filled outer shell to become stable.

a)

atoms will gain

b)

atoms will lose

c)

will share

d)

will do nothing

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