Chemistry: Periodic Table, Bonding, and Reactions Flashcards

Comprehensive vocabulary flashcards covering the periodic table, chemical bonding models (ionic, metallic, covalent), naming conventions, and types of chemical reactions based on lecture test materials.

Metal

Good conductor of heat and electric current.

Halogen

Any nonmetal in Group 7A.

Inner transition metal

An element whose highest occupied s sublevel and a nearby f sublevel contain electrons.

Representative element

An element whose highest occupied s or p sublevels are partially filled.

Ionization energy

The energy needed to remove an electron from an atom in the gaseous state.

Alkaline earth metal

An element in Group 2A.

Cation

Positively charged ion.

Electronegativity

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

Transition metal

An element whose highest occupied s sublevel and a nearby d sublevel contain electrons.

Noble gas

An element in which the highest occupied s and p sublevels are filled.

Electron dot structure

A depiction of valence electrons around the symbol of an element.

Ionic compound

Compound of cations and anions.

Valence electron

An electron in the highest occupied energy level of an atom.

Ionic bond

The force of attraction binding oppositely charged ions together.

Chemical formula

Shows the kinds and numbers of atoms in the smallest representative unit of a substance.

Halide ion

An anion of a halogen.

Alloy

A mixture of two or more elements, at least one of which is a metal.

Octet rule

Atoms in most compounds tend to achieve the electron configuration of a noble gas.

Formula unit

Lowest whole-number ratio of ions in an ionic compound.

Coordination number

The number of ions of opposite charge surrounding each ion in a crystal.

Metallic bond

The attraction of valence electrons for positive metal ions.

Covalent bond

A bond where atoms are held together by sharing electrons.

Molecule

A neutral group of atoms joined together by covalent bonds.

Diatomic molecule

A molecule that contains two atoms.

Molecular compound

A compound composed of molecules.

Molecular formula

The chemical formula of a molecular compound that shows how many atoms of each element a substance contains.

Single covalent bond

Two atoms held together by sharing one pair of electrons.

Structural formula

Represents the covalent bonds as dashes and shows the arrangement of covalently bonded atoms.

Unshared pair

A pair of valence electrons that is not shared between atoms; also known as a lone pair or a nonbonding pair.

Double covalent bond

A bond that involves two shared pairs of electrons.

Triple covalent bond

A bond formed by sharing three pairs of electrons.

Coordinate covalent bond

A covalent bond in which one atom contributes both bonding electrons.

Polyatomic ion

A tightly bound group of atoms that has a positive or negative charge and behaves as a unit.

Bond dissociation energy

The energy required to break the bond between two covalently bonded atoms.

Resonance structures

Structures that occur when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion.

Nonpolar covalent bond

A bond where the atoms in the bond pull equally and bonding electrons are shared equally.

Polar covalent bond

A covalent bond between atoms in which the electrons are shared unequally.

Dipole

A molecule that has two poles.

Van der Waals forces

The two weakest attractions between molecules, consisting of dipole interactions and dispersion forces.

Dispersion forces

The weakest of all molecular interactions, caused by the motion of electrons.

Hydrogen bonds

Attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom.

Network solid

Solids in which all of the atoms are covalently bonded to each other, resulting in very high melting points.

Anion

Any atom or group of atoms with a negative charge.

Law of definite proportions

In all samples of the same chemical compound, the elements are always combined in the same proportion by mass.

Acid

A compound that produces hydrogen ions when dissolved in water.

Base

A compound that produces hydroxide ions when dissolved in water.

Law of multiple proportions

When two elements combine to form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers.

Monatomic ion

Consists of a single atom with a positive or negative charge.

Binary compound

A compound composed of two different elements.

Coefficient

A whole number that appears before a formula in an equation.

Spectator ion

A particle not directly involved in a chemical reaction.

Combustion reaction

A reaction in which oxygen reacts with another substance, often producing heat or light.

Reactant

A starting substance in a chemical reaction.

Skeleton equation

A chemical equation that does not indicate relative amounts of reactants and products.

Balanced equation

An equation in which each side has the same number of atoms of each element.

Activity series

A list of metals in order of decreasing reactivity.

Product

A new substance formed in a chemical reaction.

Decomposition reaction

A reaction in which a single compound is broken down into simpler substances.

Single-replacement reaction

A reaction in which the atoms of one element replace the atoms of a second element.

Catalyst

A substance that speeds up a reaction but is not used up in the reaction.