AP Chem Units 1-4 MCQ

Polar

Polar

the greater the difference in position on the periodic table (especially moving up and to the right), the more polar the bond will be

Nonpolar

a type of bond where the electrons are shared equally between the two atoms, resulting in no charge separation.

Pure Substance

A material composed of only one type of particle, which can be either an element or a compound, and has consistent properties throughout.

Average Atomic Mass

the weighted average of the masses of an element's isotopes, taking into account their relative abundances.

Kinetic Molecular Theory

a theory that describes the behavior of gases in terms of particles in constant motion, explaining properties like pressure and temperature.

Gas Particles

are in constant random motion and collide elastically with each other and the walls of their container, influencing pressure and temperature.

Law Of Definite Proportion

states that a chemical compound contains its constituent elements in fixed ratio by mass, regardless of the sample size or source.

Coulomb’s Law

the attractive between two charged objects is directly proportional to the product of the charges and inversely proportional to the square of the distance between them

Aufbau Principle

states that electrons occupy the lowest energy orbitals first before filling higher ones.

Hund’s Rule

each subshell should have one electron before any subshell is filled with a second electron

Ionic Bond

always involves the transfer of electrons from the least electronegative to the most. traditionally between metal and nonmetal

Analogous Compounds

Compounds that have similar structures or functions but different compositions, often resulting in similar chemical behavior.

Electronegativity

A measure of an atom's ability to attract and hold electrons in a chemical bond.

Ionic Substances

form crystals, conduct electricity when dissolved in water, are good insulators, and have high melting and boiling points.

Metallic Substances

characterized by high electrical and thermal conductivity, malleability, ductility, and a shiny appearance.

Properties of Non-Metals

are typically brittle, poor conductors of heat and electricity, and have lower melting and boiling points

Covalent Bonds

bonds between two non-metals that involve the sharing of electron pairs to achieve stability and they occur at the lowest energy state resulting in strong attractions

Bond Energy

the amount of energy required to break a bond between two atoms in a molecule, reflecting the strength of the bond.

Larger Atomic Radii

the larger the bond length and the less bond energy due to increased distance between nuclei, leading to weaker attractions between atoms.

Lattice Energy

larger charges result in more attraction result in more energy required to separate the ions

smaller radii result in more attraction result in more energy required to separate the ions

Cations

positively charged ions that have more protons than electron

Anions

negatively charged ions that have more electrons than protons

Delocalized Electron

an electron in an atom, ion, or molecule that is not connected to a single atom or covalent bond

Interstitial Alloy

small atoms fill the spaces between the larger metal atoms in a metallic lattice

Substitutional Alloy

some of the atoms in the metallic lattice are replaced/substituted by different atoms of similar size

Miscibility

the ability of two substances to mix without separating

Intermolecular Forces

an attractive force that arises between the positive components (or protons) of one molecule and the negative components (or electrons) of another molecule.

Dipole Dipole Interactions

between two polar molecules

Ion Dipole

between and ion and a polar molecule

Ion-Induced Dipole

between ion and dispersion

Dipole-Induced Dipole

between a polar molecule and dispersion

Dispersion

a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles

Chromatography

method of separating mixtures based upon polarity differences

Paper Chromatography

most used chromatography- uses paper and water to make different colors go up

Thin Layer Chromatography

method of chromatography mostly used with amino acids

Column Chromatography

method of chromatography using a burette (the polar parts move the slowest)

Distillation

separates mixtures based on boiling points

Solubility

extent to which a solute will dissolve into a solvent from a solution

Water

good solvent, highly polar, and H20

Hydration

the process where water molecules surround the ions and dissolve them

Miscible

two substances can mix

Immiscible

two substances cannot mix

Beer-Lambert Law

states that there is a linear relationship between the concentration and the absorbance of the solution, which enables the concentration of a solution to be calculated by measuring its absorbance

Physical Process

change in properties not composition

Chemical Process

change in composition