Bonding Test Review

Types of Bonds

100

This type of bond forms when electrons are transferred from a metal to a nonmetal.

ionic bond

200

This type of bond forms when two nonmetals share electrons.

covalent bond

300

This type of bonding occurs between metal atoms and involves a “sea of electrons.”

metallic bonding

400

These two properties are typical of substances with metallic bonding.

conductivity and malleability (or ductility)

500

Compared to covalent compounds, ionic compounds typically have this property related to melting point.

a higher melting point

Valence Electrons & Octet Rule

100

The number of electrons in the outer shell of an atom.

valence electrons

200

This rule states that atoms tend to gain, lose, or share electrons to obtain 8 valence electrons.

The octet rule

300

This common element has 6 valence electrons.

oxygen

400

These elements already satisfy the octet rule without bonding.

noble gases

500

Calcium has two valence electrons and will typically form this ion. 

Ca²⁺

Lewis Dot Structures

100

These diagrams use dots around element symbols to represent valence electrons.

Lewis dot structures (diagrams)

200

In a Lewis structure, a pair of shared electrons between atoms represents this.

a covalent bond

300

The number of valence electrons shown for sulfur in a Lewis dot diagram.

6

400

The Lewis structure of O₂ contains this type of bond.

a double bond

500

This molecule has 16 total valence electrons and forms a single bond between two identical atoms with three lone pairs on each.

Cl₂

Naming & Writing Formulas

100

The name of NaCl.

sodium chloride

200

The formula for magnesium nitrate.

Mg(NO₃)₂

**It is an ionic compound composed of one magnesium ion (Mg²⁺) and two nitrate ions (NO₃^-)

300

The name of FeCl₃

iron (III) chloride -OR- ferric chloride

400

The formula for calcium phosphate.

What is Ca₃(PO₄)₂

** It is an ionic compound composed of three calcium ions (Ca²⁺) and two phosphate ions (PO₄^3-).

500

The formula for ammonium sulfate.

(NH₄)₂SO₄

** It is an inorganic salt consisting of two ammonium ions (NH₄⁺) and one sulfate ion (SO₄^2-), designed to balance the overall charge to zero.

Molecular Shape & Polarity

100

This molecule shape has two bonding pairs and no lone pairs on the central atom.

Example: O₂

linear

200

This shape has three bonding pairs around the central atom.

ex: SO₃

trigonal planar

300

A molecule with unequal electron sharing and partial charges is called this.

polar molecule

400

Even though the bonds are polar, this common molecule is nonpolar because of its symmetrical (linear) shape.

CO₂

500

This molecule is polar because of its bent shape and unequal charge distribution.

H₂O