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Periodic Law

Total questions: 70

Worksheet time: 1hrs 21mins

Name
Class
Date
1.
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
2.
Who arranged the first periodic table.
a)
Mosely
b)
Einstein
c)
Mendeleev
d)
Bohr
3.
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
4.
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.
5.
Each column in the periodic table is called a 
a)
period
b)
group
c)
cluster
d)
unit
6.

Who discovered a way to measure atomic number?

a)

John Newland

b)

Johann Dobereiner

c)

Henry Moseley

d)

Antoine Lavoisier

7.

How many periods does the Periodic Table have?

a)

18

b)

10

c)

7

d)

8

8.

Which accurately describes nonmetals?

a)

Poor conductors of electricity

b)

Often used in computer parts

c)

Both malleable and ductile

d)

Both dull and brittle

9.

Name group 18 on the periodic table.

a)
alkali metals
b)
alkaline earth metals
c)
transition metals
d)
noble gases
10.

An element that has the electron [Ne]3s23p5 is in Period

a)

2

b)

3

c)

5

d)

7

11.

An element that has the electron configuration [Ne]3s23p5 is in Group

a)

2

b)

5

c)

7

d)

17

12.

Elements in the s and p blocks of the periodic table are called

a)

alloys

b)

main-group elements

c)

metals

d)

transition metals

13.

Elements in Group 18 have

a)

very low reactivity

b)

good conductivity

c)

very high reactivity

d)

metallic character.

14.

The outer-level electron configuration of a neutral alkaline-earth metal atom consists of

a)

one electron is the s orbital

b)

two electrons in the s orbital

c)

one electron in the p orbital

d)

two electrons in the p orbital

15.

In nature the alkali metals are found only in compounds because they

a)

have small atoms.

b)

are very reactive elements.

c)

are rare elements.

d)

each have a stable octet.

16.

An element found in groups 3-12 of the periodic table is classified as a(n)

a)

alkali metal

b)

alloy

c)

transition metal

d)

actinide

17.

What block is Sulfur in?

a)

s

b)

p

c)

d

d)

f

18.

Potassium has how many electrons in it's outermost s orbital?

a)

0

b)

1

c)

2

d)

3

19.

The noble gases (except for He) has a valence electron configuration of:

a)

s2p4

b)

s2p5

c)

s2p6

d)

s2p7

20.

The lanthanides and actinides belong to the:

a)

p block

b)

d block

c)

f block

d)

s block

21.

Which of the following is the electron configuration for calcium?

a)

1s22s22p63s2

b)

1s22s22p63s23p64s2

c)

1s22s22p6

d)

1s22s22p63s23p4

22.

Which of the following is an electron configuration for a lithium atom?

a)

1s22s1

b)

1s12s21s12s2

c)

2s11s2

d)

None of the above

23.

How many valence electrons do alkali metals have?

a)

2

b)

4

c)

1

d)

3

24.

Element A is an alkaline earth metal. If element A loses two electrons to gain a complete octet, it has the same number of electrons as a(n)

a)

Halogen

b)

Alkali metal

c)

Transition metal

d)

Noble gas

e)

Alkaline earth metal

25.

if "n" stands for a given principal energy level, what is the outer electron configuration of the alkaline earth metals?

a)

ns1

b)

ns2np1

c)

ns2np5

d)

ns2

26.

Which statement correctly describes the reactivity of the alkaline earth metals compared to alkali metals?

a)

They are more reactive than the alkali metals

b)

They are less reactive, so they can be found in nature as pure elements.

c)

The reactivity is about the same.

d)

They are less reactive, but still are found in nature only as compounds.

27.

Elements in group 1 all have an electron configuration that end in

a)

s1

b)

s2

c)

s3

d)

p6

28.

Elements in group 3 all have an electron configuration that end in

a)

s1

b)

d1

c)

d2

d)

p1

29.

In general, the electron configuration of the atom's highest occupied energy level governs the atoms's chemical properties.

a)

true

b)

false

30.

The electron configuration for group 17 elements always ends in

a)

p4

b)

p5

c)

p6

d)

none of these

31.

The distance from the nucleus of an atom to the valence electrons is the __________

a)

Atomic Radius

b)

Ionization Energy

c)

Electronegativity

d)

Electrostatic

32.

As you move across a row (period) on the periodic table, the atomic radius ______________________

a)

Increases

b)

Decreases

c)

Stays the same

d)

Explodes

33.

Ionization energy is the energy needed to _________ an electron.

a)

Fission

b)

Explode

c)

Remove

d)

Add

34.

The reason the atomic radius increases down a group is due to

a)

Greater attraction by protons

b)

More energy levels (rings)

35.

As you move across a row on the periodic table, ionization energy ______________________

a)

Decreases

b)

Increases

c)

Stays the same

36.

Which element has the highest electronegativity?

a)

F

b)

Na

c)

K

d)

Li

37.

Which group of elements has the lowest ionization energy?

a)

Group 1

b)

Group 2

c)

Group 3

d)

Group 4

38.

Which element would have the smallest atomic radius?

a)

Li

b)

Be

c)

C

d)

Ne

39.

Which element would have the largest atomic radius?

a)

Cs

b)

K

c)

Na

d)

H

40.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
41.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
42.
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. 
43.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
44.
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
45.

Which of the period 3 elements has the largest electronegativity

a)

Ar

b)

Na

c)

F

d)

Cl

46.

The element with the lowest electron affinity in Period 3 is

a)

Sodium

b)

Chlorine

c)

Potassium

d)

Argon

47.

As you move from left to right across a period, the number of valence electrons

a)

increase

b)

stays the same

c)

increases then decreases

d)

decreases

48.

How many electrons would a Nitrogen ion gain/lose?

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

49.

How many electrons would a Calcium ion gain/lose?

a)

lose 1

b)

gain 1

c)

lose 2

d)

gain 2

50.

If an atom loses electrons, the charge will be positive.

a)

true

b)

false

51.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

52.

Which substance is larger

a)

Ca

b)

Ca+2

53.

Which substance is larger

a)

Br

b)

Br-1

54.

What happens to the radius of an atom when it becomes an anion?

a)

It increases

b)

It decreases

55.

Chlorine is much more apt to exist as an anion than sodium. This is because...

a)

Chlorine has a greater ionization energy than sodium does

b)

Chlorine is bigger than sodium

c)

Chlorine is more metallic than sodium

d)

Chlorine has a greater electron affinity than sodium does

56.

Which ion below has the greatest radius?

a)

Li+

b)

Cl-

c)

K+

d)

I-

57.

Potassium is much more apt to exist as a cation than bromine. This is because...

a)

Bromine has a greater electron affinity than potassium does

b)

Bromine has a greater ionization energy than potassium does

c)

Bromine is bigger than potassium

d)

Bromine is more metallic than potassium

58.

Which gives the correct order for atomic radius for Be, Li, N, C, and Ne?

a)

Be < Li < N < C < Ne

b)

C < N < Ne < Li < Be

c)

Ne < N < C < Be < Li

d)

Li < Be < C < N < Ne

59.

Which gives the correct order for first ionization energies?

a)

Ga > Ge > Se > Br > Kr

b)

Se > Ge > Br > Ga > Kr

c)

Kr > Br > Se > Ge > Ga

d)

Br > Se > Ga > Kr > Ge

60.

Which is easiest to remove an electron from?

a)

sodium (Na)

b)

magnesium (Mg)

c)

aluminum (Al)

d)

silicon (Si)

61.

Which has the highest ionization energy?

a)

sodium (Na)

b)

magnesium (Mg)

c)

aluminum (Al)

d)

silicon (Si)

62.

Which has the highest ionization energy?

a)

chlorine (Cl)

b)

bromine (Br)

c)

iodine (I)

d)

astatine (At)

63.

Which of the following is most electronegative?

a)

Oxygen (O)

b)

Nitrogen (N)

c)

Sulfur (S)

d)

Phosphorus (P)

64.

Which of the following has the highest electronegativity?

a)

argon (Ar)

b)

chlorine (Cl)

c)

krypton (Kr)

d)

bromine (Br)

65.

Which of the following has the lowest electronegativity?

a)

sulfur (S)

b)

chlorine (Cl)

c)

selenium (Se)

d)

bromine (Br)

66.

Which element is the widest (biggest radius)?

a)

sulfur (S)

b)

chlorine (Cl)

c)

selenium (Se)

d)

bromine (Br)

67.

Identify the period and group of the element that has the electron configuration [Ne] 3s2 3p3.

a)

Period 2 group 2A

b)

Period 3 group 1A

c)

Period 3 group 3A

d)

Period 3 group 5A

68.

In what group AND period can you find this element?

a)

4th period Group 8A

b)

5th period Group 2A

c)

3rd period Group 3A

d)

4th period Group 4A

69.

How many electrons does an atom generally need in its outer level to be the most stable?

a)

4

b)

8

c)

10

d)

12

70.

Statement that when the elements are arranged by increasing atomic number, there is a periodic repetition of their chemical and physical properties

a)

Atomic theory

b)

Newton's 3 laws of motion

c)

Periodic Law

d)

Octet rule

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