Pre Ib Chem Final Vocab

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Group

Collums going left to right

Period

Rows going top to bottom

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Periodic Trends

Atomic radius

The radius of an atom; increases going top to bottom on the Periodic table

Ionization energy

measure of the difficulty in removing an electron from an atom or ion

Neutron

Neutral; found in the nucleus of atoms

Proton

Positive; Found in the nucleus of atoms

Electron

Negative; Found orbiting the nucleus of atoms

Valence Electron

Electrons on the outer most ring of atoms

Alpha Decay

nuclear decay process where an unstable nucleus changes to another element by shooting out a particle composed of two protons and two neutrons (similar to that of a helium particle)

Beta Decay

Decay in which a Proton is converted into a neutron, releasing an electron and changing and element

Gamma Decay

emission of electromagnetic radiation of an extremely high frequency i.e. very high energy, giving out excess energy in order to stabilize the unstable nucleus

Electromagnetic Spectrum

the range of frequencies of electromagnetic radiation and their respective wavelengths and photon energies

Wavelength

distance between waves of energy

Frequency

number of waves which occur over a period of time

Electron configuration

distribution of electrons of an atom

Orbital

location of an electron around an atom

Molecular Geometry

three-dimensional arrangement of the atoms that constitute a molecule

Isotope

An atom which has equal protons but differing neutrons

Reactivity

The ability of an element to interact with other elements

Dipole/Polar

Points at which a molecule has differing electronegativity

Non-polar

Compound which does not differ in electronegativity

Polarity/Partial Charge

separation of electric charge in a molecule

Ionic Bonds

chemical bond formed when one atom gives up one or more electrons to another atom

Electronegativity

the tendency for an atom of a given chemical element to attract shared electrons when forming a chemical bond

Transfer electrons

Electrons which relocate to another atom

Polyatomic Ion

ion which despite having multiple atoms, behaves as a single unit.

Cation

positively charged ion

Anion

negatively charged ion

Covalent Bond

sharing of electron pairs between atoms

Lewis Dot Structures

Visual form of drawing chemicals using letters and dots

Noble Gas

Elements on the right side of the Periodic table; unreactive and 8 Valence electrons

Structural Formula

Drawn images to depict a chemical formula visually

Octet Rule

the rule which states Bonded atoms tend to have 8 Valence electrons, that of a noble gas.

Lone Pair Electrons

pair of Valence electrons which aren't used to form a bond between atoms

Bonded Pair Electrons

2 electrons which reside in the same orbital

Unpaired Electrons

electrons which aren't paired, orbit alone

Single Bond

chemical bond involving 2 Valence electrons

Double Bond

chemical bind involving 4 Valence electrons

Triple Bond

chemical bond involving 6 Valence electrons rather than 2 or 4, having three bonds

HONC 1234

rule which states that Hydrogen has 1 bond, oxygen 2, nitrogen 3, and carbon 4.

Combustion

reaction resulting in Fuel + O2 → CO2 + H2O.

Combination

process in which chemicals combine to form a single product

Decomposition

process in which chemicals break down into smaller components

Double displacement

chemical process involving the exchange of bonds between two reacting chemical species

Single displacement

chemical reaction in which one element is replaced by another in a compound

Chemical equation

equation involving chemicals

Reactant

substance that takes part in and undergoes change during a reaction.

Product

The stuff created in a reaction

Mole

Unit of measurement used to describe having 6.02x10^23 of a substance

Avogadro's Number

6\.02x10^23 (mole)

Molar Mass

the mass in grams of one mole of a substance

Dimensional Analysis

a method used to convert one unit to a different unit