Section 2.1 Q-cards

Question 1

When do atoms bond?

Answer 1

Atoms bond when their valence electrons interact.

Question 2

Which group reacts the least?

Answer 2

Atoms with full outermost energy levels are less reactive.
Ex: Nobel gas elements.

Question 3

Why do atoms form bonds?

Answer 3

To have a full outer shell.

Question 4

What holds bonded atoms together?

Answer 4

Octet Rule

Question 5

What is the Octet Rule

Answer 5

Atoms tend to lose, gain or share electrons so they have 8 electrons in their outermost shells.
Octet rule provides an important basis on witch to predict how bonds will form.

Question 6

Ionic Bonding how it forms.

Answer 6

it is formed between metal cations and non-metal anions; electrons are transferred.
Metals lose electrons to form positively charged ions or cations.
Positive ions form when the number of electrons are less than the number of protons.
Non-metals gain electrons to form negatively charged ions or anions.
Negative ions form when the number of electrons more than the number of protons.

Question 7

Ionic compound?

Answer 7

Ionic compound- a chemical compound composed of ions that are held together by ionic bonds.
Ionic compounds must have an overall charge of zero, and the number of electrons that are lost by the metal atoms must be equal to the number of electrons gained by the non-metal atoms.

Question 8

Ionic compounds containing transition metals

Answer 8

It is not possible ot predict the number of electrons that a transition metal atom can lose from its group number.
The number of electrons that a transition metal can lose can vary.

Question 9

Formation of covalent bonds

Answer 9

Covalent bonds are formed when two nonmetal atoms share electrons, and the shared electrons in the covalent bond belong to both atoms.
A molecular compound is a chemical compound that is held together by covalent bonds.

Question 10

What are molecular compounds?

Answer 10

A molecular compound is a chemical compound that is held together by covalent bonds.
Molecular compounds consist of non-metal elements only.

Question 11

Types of covalent bonds.

Answer 11

Single bonds
Double bonds
Triple bonds

Question 12

Single bonds:

Answer 12

A covalent bond that results from atoms sharing one pair of electrons.

Question 13

Double bonds:

Answer 13

A covalent bond that results from atoms sharing two pairs of electrons.

Question 14

Triple bonds:

Answer 14

A covalent bond that results from atoms sharing three pairs of electrons.

Question 15

Bonding pair

Answer 15

a pair of electrons that is charred by two atoms, thus forming a covalent bond

Question 16

Lone pair

Answer 16

a pair of elections that is not part of a covalent bond,
When a Lewis diagram is used to portray a complete molecular compound, the diagram is called a Lewis structure.

Question 17

Polyatomic ion:

Answer 17

A molecular compound with an excess or a deficit of electrons and a charge.
Polyatomic ions usually consist of two or more atoms.
The correct diagram for polyatomic ions includes brackets, a number, and a sign.

Question 18

Positively charged Polyatomic ions

Answer 18

The only positively charged polyatomic ion is the ammonium ion.
The ammonium ion forms when the molecular compound ammonia combines with a hydrogen ion.
Ammonia has three bonded pairs and one lone pair. The hydrogen ion bonds with the lone pair to form an ammonium ion.
The ammonium ion forms ionic compounds by bonding with negatively charged ions.

Question 19

Impact of electronegativity on bond formation.

Answer 19

Electronegativity indicates the relative ability of an atom of a given element to attract shared electrons. Shared electrons constitute a covalent bond.
The concept of electronegativity applies to ionic compounds as well because the positively charged nucleus of each ion attracts the negatively charged electrons of the other ions.

Question 20

What is the scale for bonds that are ionic, polar, slightly polar, and non-polar

Answer 20

1.7 and up is Mostly ionic
0.4 to 1.7 is polar covalent
higher than 0 to 0.4 is slightly polar
0 is non-polar covalentent