ib chem definitions

all the definitions i got stuck on

ionic bonding

the electrostatic attraction between two oppositely charged ions

covalent bonding

electrostatic attraction between shared electron pair and positively charged nuclei

element

a pure substance consisting of only one type of atom, which cannot be broken down into simpler substances.

homologous series functional groups formulas

compounds with similar structures and chemical properties that share a general formula, differing by a specific unit.

alkanes: C_nH_{2n + 2}

cycloalkanes/alkenes: C_nH_2n

alkyne: C_nH_{2n - 2}

alcohols: C_nH_{2n + 2}O

carbonyl: C_nH_2nO

metallic bond

electrostatic attraction between a lattice of cations and delocalized electrons

electron affinity

the energy change that occurs when an electron is added to a neutral atom, often resulting in the formation of an anion.

• this value is negative because energy is released when the electron is added

• EA may be positive or negative depending on the atom's tendency to accept an electron. A higher electron affinity indicates a stronger attraction for additional electrons.

ionization energy

the amount of energy required to remove an electron from a neutral atom in the gas phase, forming a cation.

sublimation

the process in which a solid transitions directly into a gas without passing through the liquid phase.

• this occurs most often for noble gases because they have the smallest difference between their melting and boiling points

pressure onr ate of reaction

• an increase in pressure will move to the side of the equation with a smaller number of moles

• a decrease in pressure will move to the side equationw with a higher number of moles

heat

energy transferred between systems due to a temperature difference. It can cause a change in temperature or phase of a substance.

temperature

average kinetic energy of the particles in a substance, reflecting how hot or cold it is.

intramolecular bonding

the attractive forces that hold atoms together within a molecule, such as covalent or ionic bonds.

intermolecular bonding

forces that act between molecules, influencing physical properties such as boiling and melting points. These forces include dipole-dipole interactions, hydrogen bonding, and London dispersion forces.

bond enthalpy

the energy required to break one mole of a bond in a gaseous atoms, measured under standard conditions.

q = mc∆T

m = mass of solvent

c = specific heat capacity

T= change in temperature (°C) IN DEGREES CELSIUS

K_c is solely changed by

changes in temperature, as it represents the equilibrium constant for a reaction at a given temperature.