Shart fart chemistry art

Chemical bonding

involves changes in an atom’s outer or valence electrons.

8

The valence level holds up to ____ electrons

S and P

What sublevels does chemical bonding involve

Lewis dot

Uses dots to represent number of valence electrons

Zn2+

Only Zinc ion

Ag+

Only silver ion

Sc3+

Only Scandium Ion

Cd2+

Only cadium ion

Sn2+ and Sn4+

Tin ions

Pb2+ and Pb4+

Lead Ions

Same name as metal

How to name cations

Add -ide

How to name anions

Polyatomic ions

Group of atoms with an overall charge with most being oxyanions

Root + ate

Naming oxyanions

ite

Naming oxyanions that have less oxygen

Per

Naming oxyanions with largest number of oxygens

Hypo

Naming oxyanions with lowest number of oxygens

H3O+

Hydronium

Compounds

Formed when 2 or more atoms are chemically combined in fixed ratios

Ionic bond

Attractive force between oppositely charged ions

Ionic compound

A substance composed of a cation and anion held together by electrostatic attraction

0

What must the total charge of an ionic compound be

Solid at room temperature and high melting and boiling point

Physical characteristics of ionic compounds

Ionic lattice

Tightly packed array of alternating positive and negative charges

Formula units

The repeating pattern within an ionic lattice and the smallest number of ions necessary to form a compound

Chemical formula

Formula used to indicate types and amounts of a specific element and used to represent compositions of compounds

Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine

Elements that form diatomic molecules

Empirical formula

Formula where the smallest whole number ratio of atoms in a compound is used. Used to represent ionic compounds.

Cation then anion

Order empirical formula is written

Cation then anion

Naming ionic compounds

Covalent bond

Bond formed between nonmetals and share electrons

Molecular formula

Formula often used for covalent compounds and gives the actual number of atoms in a molecule rather than simplest ratio

Uses prefixes, element lower and farther to the left of periodic table is first, element nearer to upper right is given ide

Naming covalent compounds

Solution

A solid mixed into a liquid and is a homogenous mixture

Electrolyte solution

Aqueous solution containing dissolved ionic compounds

Solvation

When molecular compounds do not separate when dissolved and are then surrounded by water molecules

Strong electrolytes

Electrolyte that completely dissociates into ions

Strong acids and ionic compounds

Examples of strong electrolytes

Weak electrolyte

Electrolyte that dissolves mostly as molecules but partially into ions

Weak acids

Examples of weak electrolytes

Molecular compounds

Examples of non-electrolytes

Dissociation

When ionic compounds are dissolved in water and the positive and negative charges are pulled apart and surrounded by water ions

Acids

Covalent compounds that produce H+ ions in aqueous solution

HCl, HBr, HI, HNO3, H2SO4, HClO4

Examples of strong acids

H2CO3, HF

Examples of weak acids

Prefix hydro and suffix ic acid

Naming binary acids

replace with ic acid

Naming oxyacids of anions that end with ate

Oxyacid

Compounds that dissociate to form H+ and an oxyanion

replace with ous acid

Naming oxyacids of anions that end with ite

HF, HCl, HBr, HI,H2CO3, HNO3, HNO2, H2SO4, H3PO4, HC2H3O2

Common acids

Hydrofluoric acid

HF

Hydrochloric acid

HCl

Hydrobromic acid

HBr

Hydroiodic acid

HI

Carbonic acid

H2CO3

Nitric acid

HNO3

Nitrous acid

HNO2

Sulfuric acid

H2SO4

Phosphoric acid

H3PO4

Acetic acid

HC2H3O2

Balanced equation

Chemical equation where the number and type of atoms is the same for the reactants and products

Decomposition, single displacement, double displacement, synthesis/recombination

4 common types of chemical reactions

Decomposition

Single reactant forms 2 or more products

Synthesis/combination

Two reactants join together to form single product

Single displacement

Reactions where one element replaces another in a compound

Double displacement

Reactions where two compounds rearrange to form two new compounds

Reactions between metals and nonmetals

One of the most common types of synthesis reactions; forms ionic compounds; reactions tend to be intense with great heat and produces bright flames

Oxidation-reduction reaction

Example of a synthesis reaction ; chemical change when one atom loses electrons while the other gains electrons

OIL RIG

Mnemonic for redox reaction

Oxidized

An atom in a redox reaction that loses electrons is

Reduced

An atom in a redox reaction that gains electrons is

formation of a solid

Driving force of a precipitation reaction

Precipitation reaction

Type of double displacement reaction; when 2 aqueous solutions combine and form a solid (insoluble) product

Color change, formation of solid, formation of gas, emission of light, emission/absorption of heat

Common indicators of a chemical change

Combustion

Reaction where oxygen gas combines with elements/compounds to produce oxide compounds; always in water and CO2 if it’s a hydrocarbon

Molecular and ionic

The two equation styles used for chemical reactions in solutions

Charge of ions, size of ions, ways ions pack together

Solubility depends of these characteristics

Neutralization reaction

a chemical reaction where an acid and a base (or alkali) react to produce water and an ionic compound called a salt; sometimes produces a gas?

Formation of water

Driving force for neutralization reactions