Unit 1 | Lesson 4-6 | The Periodic Table (Grade 9 review)

Question 1

Who created the Periodic Table?

Answer 1

Dimitri Mendeleev

Question 2

Why are/were there gaps in the Periodic Table?

Answer 2

For future elements to be discovered

Question 3

Definition of:
Periods (on the Periodic Table)

Answer 3

The rows on the Periodic Table

Question 4

Definition of:
Groups/families (on the Periodic Table)

Answer 4

The columns on the Periodic Table

Question 5

What are the three categories of the Periodic Table?

Answer 5

1. Metals
2. Non-metals
3. Metalloids

Question 6

What is the name of the first group on the Periodic Table?

Answer 6

Alkali metals

Question 7

What are some characteristics of Alkali metals?

Answer 7

1. Extremely reactive (especially with water)
2. Soft
3. Metal

Question 8

Why are Alkali metals so reactive?

Answer 8

Due to their one Valence electron

Question 9

What is the name of the second group on the Periodic Table?

Answer 9

Alkaline earth metals

Question 10

What is the main characteristic of Alkaline earth metals?

Answer 10

Extremely reactive with oxygen and halogens (but not as reactive as Alkali metals)

Question 11

What is the name of the 7th (17) group on the periodic table?

Answer 11

Halogens

Question 12

What are some characteristics of Halogens?

Answer 12

1. Reactive
2. Non-metal
3. Almost all diatomic elements

Question 13

Definition of:
Ionization

Answer 13

The process of either gaining or losing electrons to have a full outer shell

Question 14

Definition of:
Ion

Answer 14

An electrically charged atom or group of atoms

Question 15

What are the two kinds of ions and their charges?

Answer 15

Cations (+)
Anions (-)

Question 16

Definition of:
Cations

Answer 16

Positively charged ions that most commonly form when metals lose electrons

Question 17

Definition of:
Anions

Answer 17

Negatively charged ions that most commonly form when non-metals gain electrons

Question 18

How are ions formed?

Answer 18

When metals and non metals form ionic compounds

Question 19

Definition of:
Valence electrons

Answer 19

The electrons located in the outermost energy level of an atom

Question 20

How can we determine the amount of valence electrons an atom has?

Answer 20

The group number the atom is located in.

Question 21

What is the Octet Rule?

Answer 21

Atoms will bond in such a way as to have 8 electrons in their outermost energy level

Question 22

How are ionic compounds formed?

Answer 22

When electrons transfer from one atom to another

Question 23

What two kinds of elements are involved in an ionic compound?

Answer 23

A metal and a non-metal

Question 24

Properties of ionic compounds

Answer 24

• Solid at room temperature
• Dissolve in water
• Conduct electricity

Question 25

How do you properly name an ionic compound?

Answer 25

The cation is named first with the elements name, and the anion is named second with the end of its name changed to “ide”

Question 26

Definition of:
Multivalent elements

Answer 26

Elements with more than one stable ion

Question 27

Definition of:
Polyatiomic ions

Answer 27

Ions usually made up of two or more non-metals joined together

Question 28

True or False:
You have to change the anion name in a ionic compound even if it’s a polyatomic ion

Answer 28

False:
If the anion is a polyatomic ion, the ending should not be changed

Question 29

Definition of:
Molecular compounds

Answer 29

Compounds that form through 2 non-metals

Question 30

True or False:
Molecular compounds can only be solid

Answer 30

False:
Molecular compounds can be either a solid, liquid, or gas

Question 31

What’s the difference(s) between an ionic compound and a molecular compound

Answer 31

1. Ionic compounds are made from a metal and a non-metal, while a molecular compound is made from 2 non-metals
2. Ionic compounds dissolve in water while molecular usually do not
3. Ionic compounds are solid at room temperature, while molecular compounds can be solid, liquid, or gas