AICE Chemistry Vocabulary

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Halogens

Group 17 elements

Proton

Mass: 1amu
Charge: +1
Charge/C: +1.6x10^-19
Electron Field Behavior: Move towards negative plate

Neutron

Mass: 1amu
Charge: 0
Charge/C: 0
Electron Field Behavior: Move straight

Electron

Mass: 1/1836amu
Charge: -1
Charge/C: -1.6x10^-19
Electron Field Behavior: Move towards positive plate

Proton/Atomic Number

Total number of protons in the nucleus

Nucleon/Mass Number

Total number of protons and neutrons in the nucleus

Cation

A positively charged ion

Anion

A negatively charged ion

Isoelectronic

Having the same number of electrons

Isotonic

Having the same number of neutrons

Isotopic

Having the same number of protons

Isotopes

Atoms with the same number of protons but different numbers of neutrons

Isotopes have the same:

Number of protons and electrons
Electronic Configuration
Chemical Properties

Isotopes have different:

Number of neutrons and nucleon number
Mass
Density
Molecular speed

Radioisotopes

Unstable isotopes

Relative Mass (amu)

Mass of an atom compared to one atom of carbon-12

Relative Isotopic Mass

The mass of an isotope compared to an atom of carbon-12

Relative Atomic Mass (Ar)

Average mass of one atom of the element / mass of one atom of carbon-12 X 12

Relative Molecular Mass (Mr)

The weighted average of the masses of molecules

Relative Formula Mass (Mr)

The weighted average of the masses of the formula units

Mass Spectrometer

An instrument that is used to determine:

Relative isotopic, atomic, and molecular mass
Relative abundance of isotopes
Structural formula of compounds

Vaporization

Step 1:
Atoms are vaporized to form gaseous atoms

Ionization

Step 2:
Gaseous atoms are struck with high energy electrons to create positive ions

Acceleration

Step 3:
Ions are accelerated to have the same kinetic energy

Deflection

Step 4:
Ions are deflected by a magnetic field

Detection

Step 5:
The ions are electronically detected, and the mass spectrum is produced

Mass Spectrum

A graph of the data from a mass spectrometer, where m/z ratios of the deflected particles are plotted against the number of particles with a particular mass

Avogadro's Constant (L)

1 mol \= 6.02X10^23 molecules

Room Temperature (RTP)

Temperature: 20 C
Pressure: 1 atm
Volume: 24 dm^3

Standard Temperature and Pressure (STP)

Temperature: 0 C
Pressure: 1 atm
Volume: 22.4 dm^3

Avogadro's Law

Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules

Number of Moles of Gas

Volume of gas (dm^3) / molar volume (dm^3 mol^-1)

Solution

A homogeneous mixture of two or more substances

Solute

A substance that is dissolved in a solution.

Solvent

A liquid substance capable of dissolving other substances

Concentration (g dm^-3)

A measurement of how much solute exists within a certain volume of solvent

Molarity

Concentration (g dm^-3) / molar mass of solute (g mol^-1)

Percent Composition by Mass

Ar / molar mass X 100

Empirical Formula

A chemical formula with the simplest ratio of atoms

Molecular Formula

A chemical formula with the actual number of atoms

Principle of Conservation of Mass

During a chemical reaction, matter is not created or destroyed

Stoichiometry

The relationship between the relative quantities of substances taking part in a reaction; a ratio

Net Ionic Equation

An equation for a reaction in a solution showing only those particles that are directly involved in the chemical change

Quantum Shell

The rings where electrons are found

Quantum Subshells

Divisions of quantum shells

S < P < D < F

Heisenberg Uncertainty Principle

It is impossible to know exactly both the velocity and the position of a particle at the same time

Atomic Orbital

A region of space in which there is a high probability of finding an electron

S Orbital

Spherical and non-directional

P Orbital

Dumbbell shaped and directional

Electron Configuration

The arrangement of electrons in an atom

Aufbau Principle

An electron occupies the lowest-energy orbital that can receive it

Pauli's Exclusion Principle

No more than two electrons of opposite spin can occupy a given orbital.

Hund's Rule

Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin

Electron Configuration of K

1s2 2s2 2p6 3s2 3p6 4s1

4s has a lower energy level than 3d

Electron Configuration of Sc

1s2 2s2 2p6 3s2 3p6 4s2 3d1

The energy levels of 3d and 4s are reversed

Electron Configuration of Cr

1s2 2s2 2p6 3s2 3p6 4s1 3d5

Fully filled or half-filled orbitals are extra stable

Electron Configuration of Cu

1s2 2s2 2p6 3s2 3p6 4s1 3d10

Fully filled or half-filled orbitals are extra stable

Ionisation Energy (kJ mol^-1)

The energy required to remove a mole of electrons from a mole of isolated gaseous atoms or ions.

Shielding Effect

A constant effect when new electrons feel more positive charge as more protons are added to the nucleus, but outer layers feel less positive charge because they are shielded by the inner layers.

Ionic Bond

Formed when one or more electrons are transferred from one atom to another

Very strong
Non-directional

Lewis Dot Diagram

Diagram of an atom, ion or molecule in which each dot represents a valence electron

Covalent Bond

A chemical bond that involves sharing a pair of electrons between atoms in a molecule

Lone Pair

A pair of electrons that is not involved in bonding and that belongs exclusively to one atom

Octet Deficient

An atom that has less than eight electrons

Expanded Octet

An atom that has more than eight electrons

Co-Ordinate Bond

A covalent bond in which both electrons in the shared pair come from the same atom.

Valence Shell Electron Pair Repulsion (VSEPR) Theory

All electron pairs will repel each other

Linear

Two bonded
180 degrees
Nonpolar

Bent

Two bonded
One to two lone pairs
104.5 degrees
Polar

Trigonal Planar

Three bonded
120 degrees
Nonpolar

Trigonal Pyramidal

Three bonded
One lone pair
107 degrees
Polar

Tetrahedral

Four bonded
109.5 degrees
Nonpolar

Trigonal Bipyramidal

Five bonded
90-120 degrees
Polar

Octahedral

Six bonded
90 degrees
Nonpolar

Sigma Bond (σ bond)

Bond formed directly between two atoms by the head on overlap of orbitals

Pi Bond (π-bond)

Covalent bond formed by side-by-side overlap of atomic orbitals

Hybridization

The mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals

sp3 Hybridization

The formation of a hybrid orbital from one 2s and three 2p orbitals

sp2 Hybridization

s, p, p orbital and 3 hybrid orbitals, trigonal-planar

sp Hybridization

The 2s orbital mixes with only one of the three p-orbitals resulting in two sp orbitals and two remaining unchanged p orbitals

Electronegativity

The ability of an atom to attract electrons when the atom is in a compound

Dipole Moment

The product of charges and the distance between the centre of the charges

Bond Length

The average distance between two bonded atoms

Bond Energy

The energy required to break a chemical bond

Intramolecular Forces

Bonding forces that hold the atoms of a molecule together

Intermolecular Forces

Forces of attraction between molecules

Dipole-Dipole Forces

Attractions between oppositely charged regions of polar molecules

London Dispersion Forces (LDF)

The weakest forces that result from temporary shifts in the density of electrons in electron clouds

Hydrogen Bonding

The strongest type of intermolecular dipole-dipole attraction between hydrogen and F, O, or N

Metallic Bond

An attraction between a positive metal ion and the electrons surrounding it

Delocalized Electrons

Electrons that are free to move

Kinetic Theory of Gases

Assumes that gas molecules are small compared to the distance between then and that they are in constant random motion

Ideal Gas

A hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory

Ideal Gas Equation

PV \= nRT

Boyle's Law

P1V1\=P2V2

Charles' Law

V1/T1\=V2/T2

Kinetic Theory of Liquids

A liquid takes the shape of its container because particles in a liquid can flow to new locations, and forces of attraction keep the particles close together

Maxwell-Boltzmann (Energy Distribution) Curve

A graph of energy against the number of particles in a sample with those energies

Vapor Pressure

The pressure exerted by a vapor over a liquid

Equilibrium

A state in which reactants are forming products at the same rate that products are forming reactants