Unit 3 Chemical Bonding Test Review

Vocabulary flashcards covering chemical bonding concepts, periodic table trends, naming ionic and covalent compounds, formulas, and oxidation numbers from Unit 3.

Properties of metals

Physical characteristics including being solid at room temperature (except mercury), ductile, malleable, having luster (reflecting light), and conducting heat and electricity.

Ductile

The property of metals that allows them to be drawn or pulled into wires.

Luster

The ability of metals to reflect light.

Transition elements

The metallic elements located in Groups $3$ through $12$ of the periodic table.

Alkaline earth metals

The family of elements in Group 2 of the periodic table that possesses two electrons in its outer energy level.

Mercury

The only metallic element that exists as a liquid at room temperature.

Metalloids

Elements that lie along the stair-step line of the periodic table, possessing properties intermediate between metals and nonmetals.

Group 12 transition elements

The transition metals located in Group $12$: zinc ($Zn$), cadmium ($Cd$), and mercury ($Hg$).

Chemical formula

A notation using chemical symbols and numerical subscripts to show the elements that make up a compound and the number of atoms of each element in a unit of the compound.

Covalent bond

A chemical bond formed when two or more atoms share electrons.

Polar covalent bond

A type of covalent bond in which electrons are shared unequally between atoms.

Ionic bond

A chemical bond formed when electrons are transferred from one atom to another, creating oppositely charged ions that attract.

Oxidation number

The positive or negative number assigned to an element indicating how many electrons an atom gains, loses, or shares to become stable.

Chemically stable outer level

The condition where an atom has $8$ electrons in its outer energy level, fulfilling the octet requirement for stability.

Lithium fluoride

The binary ionic compound formed between the alkali metal lithium ($Li$) and the halogen fluorine ($F$).

Lithium chloride

The binary compound formed from lithium ($Li$) and chlorine ($Cl$).

Subscript in $MgCl_2$

The numeral $2$ that indicates there are two chloride ions for every one magnesium ion in the ionic formula unit.

Copper(II)

Nomenclature indicating that the copper ion in the compound has an oxidation state or charge of $2+$.

Beryllium chloride ($BeCl_2$)

The binary ionic compound formed by beryllium and chlorine in a $1:2$ ratio of beryllium ions to chloride ions.

Carbon dioxide prefix

The prefix 'di-' in the second word indicating that each molecule of the compound contains two oxygen atoms.

Sum of oxidation numbers

A fundamental chemical rule stating that the total sum of the oxidation numbers in a neutral compound is always $0$.

Noble gases

Group 18 elements that do not form compounds readily because their outer energy levels are completely full and stable.

Sodium chloride ($NaCl$)

The binary ionic compound formed from sodium ($Na^+$) and chlorine ($Cl^-$).

Hydrogen count in ammonium acetate ($NH_4C_2H_3O_2$)

A total of $7$ hydrogen atoms present in one molecule ($4$ from the ammonium group and $3$ from the acetate group).

Magnesium nitrate

The ionic compound formed from magnesium ($Mg^{2+}$) and nitrate ($NO_3^-$) with the chemical formula $Mg(NO_3)_2$.

Phosphate ion in $K_3PO_4$

The polyatomic ion ($PO_4^{3-}$) carrying an ionic charge and oxidation state of $3-$.

Potassium oxide ratio

A binary compound ($K_2O$) containing two potassium atoms for every one oxygen atom.

Potassium sulfate ($K_2SO_4$)

The ionic compound consisting of two potassium cations ($K^+$) bonded to one polyatomic sulfate anion ($SO_4^{2-}$).

Magnesium oxide ($MgO$)

The ionic compound formed in a $1:1$ ratio between magnesium ($Mg^{2+}$) and oxygen ($O^{2-}$).

Aluminum oxide ($Al_2O_3$)

The ionic compound in which aluminum has an oxidation number of $3+$ and oxygen has an oxidation number of $2-$.

Sodium sulfate formula

The chemical formula $Na_2SO_4$, balancing two sodium ions ($Na^+$) with one sulfate polyatomic ion ($SO_4^{2-}$).

Oxidation number of oxygen in $H_2O$

The oxidation state of oxygen in water, which is $-2$.

Dihydrogen dioxide ($H_2O_2$)

The systematic covalent chemical name for hydrogen peroxide, indicating a molecule with two hydrogen atoms and two oxygen atoms.

Oxidation number of nonmetal in $K_2O$

The oxidation state of the oxygen anion in potassium oxide, which is equal to $-2$.