Chem Chapter 3

Front 1

Two types of chemical bonds

Back 1

Ionic and covalent

Front 2

Definition: Ionic bond

Back 2

Bond between a metal and one or more nonmetals. Forms cations and anions. Complete transfer of electrons. Oppositely charged ions are attracted.

Front 3

Definition: Cation

Back 3

A positively charged ion

Front 4

Definition: Anion

Back 4

A negatively charged ion

Front 5

Definition: Covalent bond

Back 5

Bond between nonmetals. Sharing of electrons. Form molecules.

Front 6

Definition: Molecular compounds

Back 6

Covalently bonded compounds, usually between nonmetals.

Front 7

Order of elements in a chemical formula for a compound

Back 7

More metallic (positively charged) first, less metallic second.

Front 8

Types of chemical formulas

Back 8

Empirical, molecular, and structural

Front 9

Definition: Empirical formula

Back 9

Gives the relative number of atoms in a compound

Front 10

Definition: Molecular formula

Back 10

Gives the actual number of atoms in a compound

Front 11

Definition: Structural formula

Back 11

Uses lines to represent covalent bonds, and may show the compound's geometry

Front 12

Types of pure substances

Back 12

Elements and compounds

Front 13

Types of elements

Back 13

Atomic and molecular

Front 14

Types of compounds

Back 14

Molecular and ionic

Front 15

Definition: Atomic elements

Back 15

Exist with single atoms as their basic units.

Ex: Ne

Front 16

Definition: Molecular elements

Back 16

An element that normally exists as a molecule.
Ex: 02

Front 17

List of diatomic elements

Back 17

H, N, O, F, Cl, Br, I

Front 18

List of polyatomic elements

Back 18

P (4), S (8), Se

Front 19

Definition: Formula unit

Back 19

The smallest, electrically neutral collection of ions in an ionic compound. Same as the empirical formula

Front 20

Definition: Polyatomic ion

Back 20

An ion composed of two or more atoms.

Ex: Hypochlorite, ClO -

Front 21

Rule: Writing formulas for ionic compounds

Back 21

1. Write the cation first and anion second with superscripts for charge. (use P-table)

2. Adjust the subscripts to balance the charges.

Ex: Al 3+ and O 2- gives Al2O3

Front 22

Two branches for naming ionic compounds

Back 22

1. Metal forms ions with only one charge (no numeral)

2. Metal forms variably charged ions (use numeral)

Front 23

Rule: Naming ionic compounds with metals that form only one charge of ion

Back 23

Name of cation, base name of anion +ide.

Front 24

Which metals have invariably charged ions?

Back 24

Main group metals with the exception of Tin (Sn) and Lead (Pb). Charge determined by the group number.

Front 25

Definition: Binary compound

Back 25

Contains only two different elements.

Front 26

Rule: Naming binary ionic compounds with metals that form variably charged ions

Back 26

Name of cation (roman numeral for cation charge), base name of anion +ide.

Ex: CrBr3 chromium (III) bromide

Front 27

Which metals form ions with variable charges?

Back 27

The transition metals. Charge determined by what they are bonded to. Exceptions are zinc (Zn) 2+, silver (Ag) +, cadmium (Cd) 2+, and scandium (Sc) 3+

Front 28

Rule: Naming ionic compounds containing polyatomic ions

Back 28

Name the metal with roman numeral if needed, then name the polyatomic ion.

Ex: NaNO2 sodium nitrite, FeSO4 iron (II) sulfate

Front 29

Prefixes and endings for oxyanions, from least to most O's

Back 29

hypo___ite

___ite

___ate

per___ate

Front 30

Definition: Hydrates

Back 30

Ionic compounds that contain a specific number of water molecules associated with each formula unit.

Ex: MgSO4⋅7H2O

Front 31

Definition: Anhydrates

Back 31

A salt with no water trapped inside the crystal lattice.

Front 32

Definition: Waters of hydration

Back 32

The water molecules trapped within the crystal lattice of a salt.

Front 33

To determine the number of waters of hydration in an ionic hydrate divide ______ by ______.

Back 33

The moles H20

The moles of the metal

Front 34

Rule: Naming hydrates

Back 34

Name the ionic compound according to ionic compound rules then prefixhydrate.
Ex: BaCl2⋅6H2O barium chloride hexahydrate

Front 35

List of prefixes

Back 35

Hemi 1/2, Mono 1, Di 2, Tri 3, Tetra 4, Penta 5, Hexa 6, Hepta 7, Octa 8, Nona 9, Deca 10

Front 36

Rule: Naming molecular compounds

Back 36

Prefix, 1st element name + prefix, 2nd element name. (more metallic element is first) (if the prefix of the first is mono it can be dropped)

Ex: NO2 nitrogen dioxide

Front 37

Definition: Acids

Back 37

Molecular compounds that release hydrogen ions when dissolved in water. Formula starts with H

Front 38

Two types of acids when naming

Back 38

Binary (contains two elements) and oxyacids (contain oxygen)

Front 39

Rule: Naming binary acids

Back 39

Hydro, base name of nonmetal +ic, acid

Ex: HCl(aq) hydrochloric acid

Front 40

Rule: Naming oxyacids

Back 40

1. Oxyanion ends in -ate. Take base name of oxyanoion +ic acid

2. Oxyanion ends in -ite. Take base name of oxyanion +ous acid

Ex: HNO3(aq) nitric acid, H2SO3(aq) sulfurous acid

Front 41

Definition: formula mass / molecular mass / molecular weight

Back 41

The average mass of a molecule or formula unit of a compound.

Front 42

Finding formula mass

Back 42

# of 1st atom x atomic mass of 1st atom + # of 2nd atom x atomic mass of 2nd atom + ...

Front 43

Definition: Molar mass of a compound

Back 43

The mass in grams of one mole of a compound. Same number as the formula mass, but in g.
Ex: CO2 molar mass= 44.01 g/mol

Front 44

Definition: Mass percent

Back 44

The percent of an element's mass of the compound's total mass.

Front 45

Finding mass percent

Back 45

(mass of element in 1 mol of compound)/(mass of 1 mol of the compound) all x 100%

If the element has a subscript, multiply it in the numerator.

Front 46

Conceptual plan for masses in compound

Back 46

Mass A -> Moles A -> Moles B -> Mass B

Front 47

Finding empirical formula using mass percent composition

Back 47

1. Convert masses to moles

2. Write moles as subscripts

3. Divide all by the smallest number

4. Convert decimals to smallest whole number ratios

Front 48

Finding molecular formula from empirical formula

Back 48

1. Divide molar mass by empirical formula molar mass

2. Multiply the subscripts of the empirical formula by that number

Front 49

Definition: Combustion reaction

Back 49

A chemical reaction in which a substance combines with oxygen and gives off heat.

Front 50

Two sides of a chemical equation

Back 50

Reactants/reagents and products

Front 51

Definition: Hydrocarbons

Back 51

Organic compounds that contain only one C and H

Front 52

Definition: Functional Group

Back 52

A characteristic atom or group of atoms that are incorporated into a hydrocarbon, changing its properties

Front 53

Definition: Family (in regards to organic compounds)

Back 53

A group of organic compounds with the same functional group.