Chemical Bonding: Ionic Bonds

Question 1

These elements have low chemical reactivity and are monotonic, colorless, odorless, and nonflammable. They also have little tendency to receive or lose electrons due to their complete valence electron shells, so they are incredibly stable and unlikely to form chemical bonds.

Answer 1

Noble Gases

Question 2

A rule that states that some atoms can be stable when they have two electrons in their outermost shell, or duplet. This rule applies to atoms with only one shell, which can hold a maximum of two electrons

Answer 2

Duplet rule

Question 3

A rule states that atoms with more than two electrons tend to gain, lose, or share electrons to have eight electrons in their outermost shell.

Answer 3

Octet rule

Question 4

Atoms can achieve duplet or octet electron configuration by:

Answer 4

1. Giving away excess electrons
2. Receiving electrons from another atom to complete the octet
3. Sharing electrons with another atom to form an octet

Question 5

A bonding occurs when one atom donates an electron to another atom, forming positively and negatively charged ions. The electrostatic attraction between these oppositely charged ions holds them together.

Answer 5

Ionic bonding

Question 6

The number of _______________ indicates the possible bonds and which elements could form ionic bonds with each other.

Answer 6

Valence electrons

Question 7

These elements can lose different numbers of electrons from their outermost and next-to-outermost electron shells.

Answer 7

Transition metals

Question 8

Ions consist of two or more atoms bonded together, carrying an overall charge.

Answer 8

Polyatomic ions

Question 9

Steps on how to construct a Lewis Structure

Answer 9

1. Find how many valence electrons (N) are in the molecule, which must be shown on the Lewis Structure using the periodic table. Find the charge, add an electron for every negative charge, and remove an electron for every positive charge.
2. Draw out the molecule’s single bonds and initial framework, called the skeleton.
3. Complete the octets around the non-central atoms, i.e., the terminal atoms, by using the lone pairs of electrons.
4. Compare the number of electrons currently depicted to the number needed (N) in the central atom and add electrons to it until the octet is complete.
5. If there are extra lone-pair electrons and the octet rule is not filled for the central atom, use the extra electrons to form double or triple bonds around the central atom.
6. Check the formal charge of each atom.

Question 10

The dots surrounding the chemical symbol are the (1) _________________, and each dash represents one (2) ________________. (consisting of two [2] valence electrons).

Answer 10

1. Valence electrons
2. Covalent bond

Question 11

Refers to the element that is always terminal with the structure.

Answer 11

Hydrogen

Question 12

The atom with the lowest ionization energy is typically the _________________ in the structure.

Answer 12

Central atom

Question 13

These are the positively charged ions.

Answer 13

Cations

Question 14

These are the negatively charged ions.

Answer 14

Anions

Question 15

Employing the _______________ method to predict the compound ions ratio can predict the chemical formulas.

Answer 15

Criss Cross Method