chemistry

the 14 elements with atomic numbers from 90 to 103

Actinides

forces between molecules

intermolecular forces

the bond that exists between 2 atoms in a molecule/compound

intramolecular

A positively charged ion

cation

bonds that form from the transferring of electrons and is always non metal with a metal

ionic

polyatomic ions that contain oxygen and 1 other element

oxyanions

the concept of electronegativity was developed by this American chemist in 1922

Linus Pauling

crystal lattice

the structure formed by all ionic solids(formed from the arrangment of ions

What is ionic bonding?

transfer of electrons

sharing of electrons/non metal and non metal

covalent

seeing more than one part of substance

heterogeneous

57 and the first row at the bottom. Are rare earth elements.

lanthenides

what is the concept of stoichiometry

the science of proportions in chemical reactions.

What is a quantitative observation?

An observation you make using numbers and / or measurement

What is qualitive data?

is descriptive and involves characteristics that cant be counted

Matter is not created nor destroyed in any chemical or physical change

law of conservation of matter

what is formula mass measured in

amu

the reactant that is completely used up at the end of a chemical reaction

limiting

the reactant that remains at the end of a chemical reaction

excess

the formula that represents the simplest whole number ratio of atoms of each element in one molecule of the compound

empirical

Isotope

Atoms of the same element that have different numbers of neutrons

isotopic abundance

the percentage of a given isotope in a sample of an element

nuclear radiation

energy emitted from the nucleus of a radioisotope

3 types of nuclear radiation

alpha (blocked by paper positive), beta(blocked by aluminum negative) , gamma (blocked by led high energy electromagnetic)

atomic mass

mass of the atom number of proton and neutrons

atomic radius

an estimate of the size of the atom, from inner nucleus to outer valence shell.

as you move down atomic radius

increases

as to move across a period atomic radius

decreases

ionization energy

The amount of energy required to remove an electron from an atom

as you move down a group electron affinity, ionization enegry and electronegativity

decreases

as to move across a period electron affinity, ionization enegry and electronegativity

increases

electron affinity

an atoms attraction for additional electrons

Electronegativity

the property that determines how strongly attracted the electrons in a chemical bond are between atoms.

The attraction between the slightly positive end of one polar molecule and the slightly negative end of another

dipole-dipole force

attraction between the temporary molecules; weakest involving the nucleus of the atom of molecule unit being attracted to the outer electrons of another molecule unit

London dispersion force

theoretical knowledge

knowledge that explains scientific observations

empirical observation

observation to explain ideas

What is effective nuclear charge?

nuclear protons acting on valence electrons

what is chemical bond?

the force that holds two atoms together

Examples of intramolecular bonds

ionic, polar covalent, non- polar covalent

unusually strong dipole-dipole force between a hydrogen atom attached to a highly electronegative atom (N,O OR F) and a highly electronegative atom in another molecule

hydrogen bond

whats is a electrolyte

compound that dissolves in water

ions that have more than one possible valence (ex.copper, lead)

multivalent ions

Binary ionic bonds

Binary ionic bondsCompound made up of 2 elements (non metal and metal) (ex,CaCl2- calcium chloride)

Non-binary Ionic Compounds

metal and polyatomic ion( ex. AlPO4- Aluminum phosphate)

hydrated salts

any ionic compound that includes water molecules (ex.Na2Co3.7H2O-sodium carbonate heptahydrate

acid salt

cation bonds with a acid anion

binary covalent compounds

Non metal and a non metal has charges in the name (ex.CO2- carbon dioxide

acid anion

normal metals bonded with hydrogen bonded to a polyatomic (ex.Mg(HS)2,NaHCO3,LiHSO3) make sure to criss cross and add brackets

binary acids

any compound that starts with hydrogen bonded to another non metal (ex. HCL-hydro chloric acid)

Non-binary compound

compound containing a non metal and a polyatomic ion

polyatomic ion

ions which consist of more than one atom

Ternary Acids

acids that begin with a hydrogen and end with a polyatomic ion (ex.HNO-nitric acid)

diatomic molecule

a molecule that consists of two atoms of the same element ex.H2 O2 F2 ETC name based on the state of the atom for example H2\= hydrogen gas

electrostatic force

the force of attraction between two charged atoms

Solute

A substance that is dissolved in a solution.

Solvent

A liquid substance capable of dissolving other substances

combustion reaction

a chemical reaction that occurs when a substance reacts with oxygen, releasing energy in the form of heat and light

precipitate

a solid that forms and settles out of a liquid mixture

catalyst

catalyst are materials that increase the efficiency of a reaction

acidic oxide

a covalent compound made of a non-metal element bonded to an oxygen (ex.CO2,N2O5)

basic oxide

an ionic compound made of a metal element bonded to oxygen (always solids) (ex.MgO,Na2O

acid

a covalent compound made of hydrogen bonded to either one non metal element or hydrogen bonded to a polyatomic. (ex.HCL(aq),H2SO4(aq) they produce hydrogen ioncs when dissolved, they conduct electricity, taste sour and has pH less than 7

base

a ionic compound made of a metal bonded to the hydroxide ion, produce hydroxide when dissolved, taste bitter, forms solution that conducts electricity, turns litmus paper blue. (NaOH,Ca(OH)2

salt

any neutral ionic compound that is not an acidic oxide a basic oxide an acid or base (ex.MgCl2,Ca(NO3)2)

the mole

the base unit used to measure the amount of a substance

Avogadro's number

number of representative particles in a mole, 6.02 X 10^23

homogenous

see only 1 phase

atom

smallest particle of an element

anion

negativley charged atom

horizontal on the periodic table

periods

groups

vertical columns

mass spectrometer

measuring instrument to measure the mass of a molecule after in converts to a gas ion

radioactive decay

A spontaneous disintegration of unstable isotopes

dipole

slight difference in charge that exists between atoms in a polar covalent bond

developed the theory of intermolecular forces

Johannes van der Waals

Solubility

the quantity of a solute that can dissolve in a solvent

in double displacement what are the 3 products that futher decompose into a gas and water?

Carbonic acid, Ammonium Hydroxide, Sulfurous acid

Antacids

neutralize the acids in the stomach

organic compounds

a covalent compound that contains one or more carbon-carbon bonds and often one or more carbon-hydrogen bonds.

hydrocarbon

a type of organic compound that is made up of only carbon-carbon and carbon hydrogen bonds.

air pollution

chemicals and particles in the atoms that harm living organisms or damage the environment.

2 types of combustion reactions

complete combustion and incomplete combustion

formula unit

the lowest whole-number ratio of ions in an ionic compound (ex.the formula unit of Na2Cl2 is NaCl) the smallest unit of an ionic compound

polar covalent bond

A covalent bond in which electrons are not shared equally

non polar covalent bond

a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge

anhydrous salt

A salt which contains no water of crystallisation

neutralization reaction

a reaction in which an acid and a base react in an aqueous solution to produce a salt and water

Complete combustion

combustion that occurs when there is plenty of oxygen; it produces carbon dioxide and water vapour

Incomplete combustion

When a fuel burns in insufficient oxygen, producing carbon monoxide as a toxic product.

percentage composition

the percentage by mass of each element in a compound

law of definite proportions

a given compound always contains exactly the same proportion of elements by mass

mole ratio

!a conversion factor! that relates the amounts in moles of any two substances involved in a chemical reaction

spectator ions

ions that do not participate in a reaction

reactants

A starting material in a chemical reaction found on left side

Products

The elements or compounds produced by a chemical reaction. always on right side

biochemical

The changing of organic matter into other chemical forms such as fuels.

thermal energy

Heat energy

gas production

formation of gas appearing as bubbles

Exothermic

energy releasing chemical reactions