Free Printable Unit 3 Test Review: The Periodic Table

Worksheets

Unit 3 Test Review: The Periodic Table

Total questions: 25

Worksheet time: 30mins

Name

Class

Date

On the periodic table, the horizontal rows are called

Periods

Groups

Elements

Compounds

On the periodic table, the vertical columns are called

Periods

Groups

Elements

Compounds

Elements in group 2 are called

Alkali Metals

Alkaline Earth Metals

Transition Metals

Halogens

Elements in group 3-12 are called

Alkali Metals

Alkaline Earth Metals

Transition Metals

Halogens

Elements in group 17 are called

Alkali Metals

Alkaline Earth Metals

Transition Metals

Halogens

Elements in group 1 are called

Alkali Metals

Alkaline Earth Metals

Transition Metals

Halogens

Elements in group 18 are called

Alkali Metals

Alkaline Earth Metals

Transition Metals

Noble Gases

Hydrogen (atomic number 1) would best be classified as a(n)

Alkali Metal

Alkaline Earth Metal

Transition Metal

Nonmetal

Noble gases are extremely reactive

True

False

10.

What type of elements fall along the "staircase"

Metalloids

Metals

Non-metals

Noble gases

11.

If a student observes a silvery solid that is malleable, good conductor, and ductile it is a...

nonmetal

metal

metalloid

12.

If an object breaks easily, that means it is probably-

malleable

brittle

ductile

13.

´Elizabeth was examining elements and their physical properties. She described an element is her science journal as having no shine, an insulator, and very brittle. What would this element be a metal, nonmetal, or metalloid?

metal

nonmetal

metalloid

14.

As you move down a group, atomic radius increases because -

you add more and more neutrons

you add more and more protons

you add more and more shells (energy levels)

you add more atomic mass

15.

The atom with the largest atomic radius in Group 18 is -

16.

As you move across the periodic table from left to right, the atomic radius decreases. This is because -

the number of protons increases, so attraction to electrons increases

the number of energy levels increases

the number of electrons increases

the atomic mass increases

17.

The atom with the largest atomic radius in Period 4 (row 4) is -

18.

Francium (Fr) has the lowest ionization energy in Group 1 because -

it has the smallest number of valence electrons

it has the greatest atomic mass

it has the greatest number of protons, so it attracts its electrons the strongest

its 1 valence electron is very far from the nucleus, so little energy is needed to remove it

19.

The element with the smallest ionization energy in Period 6 is -

20.

As you move across the periodic table atoms tend to get smaller because, ______________.

the atoms have more mass.

the atoms have less mass

the atoms have more protons.

the atoms have less electrons.

21.

The energy required to remove electrons is the definition of:

Electronegativity

Atomic Number

Atomic Radius

Ionization

22.

Families all have similar

Names

atomic numbers

atomic masses

properties

23.

Electronegativity is...

the ability of an atom to attract/ accept electrons

the ability of an atom to lose electrons

the energy required to remove an electron from a specific atom

how easy it is to make friends.

24.

Which has the greater Electronegativity:
N or C?

25.

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

decreases, increases

increases, increases

increases, decreases

stays the same, increases

100 %

Unit 3 Test Review: The Periodic Table

Total questions: 25

Worksheet time: 30mins

Similar Resources on Wayground