Chemistry Vocabulary 10th grade.

Ion

A charged atom

Cation

A positively charged ion

Anion

A negatively charged ion

ionic bond

Formed when one or more electrons are transferred from one atom to another; results from the attraction between oppositely charged ions

covalent bond

a chemical bond in which two or more atoms share valence electrons

double covalent bond

two pairs of electrons are shared instead of one

triple covalent bond

three pairs of electrons are shared instead of one

metallic bond

a bond formed between metals; is described as a bunch of positively charged metallic ions in a sea of negatively charged electrons

chemical bond

the attractive force that holds atoms or ions together in a compound

Metal properties

Shiny, malleable, ductile, conductive because of the sea of mobile valence electrons, high melting points because of strong attraction between the positive metal kernels and valence electrons

Nitrate

NO3- (-1 ion)

hydroxide

OH- (-1 ion)

carbonate

CO3 2-

sulfate

SO4 2-

phosphate

PO4 3-

Substance

A type of matter with a fixed composition.

Element

If all the atoms in a substance has the same identity it becomes {blank}.

Compound

A substance in which the atoms of 2 or more elements are combined.

Heterogeneous Mixture

Mixture in which different materials can easily be distinguished.

Homogeneous Mixture

Contains 2 or more gases, liquids, or solids substances blended evenly.

Solution

Homogeneous mixture with particles so small that they cannot be seen with a microscope.

Physical Property

Characteristic of a material you can observe without changing the identity.

Physical Change

A change in size, shape, or state.

Distillation

A process for separating substances by evaporating a liquid and recondensing its vapor.

Chemical Property

Characteristic of a substance that indicates whether it can undergo a chemical change.

Chemical Change

A change of one substance to another.

Law of Conservation and Mass

The mass of all substances that are present before a chemical change equals the mass of all the substances after the change.

Kinetic Theory

Explanation of how particles in matter behave.

Melting Point

The point in temperature when the solid starts to liquefy.

Boiling Point

The point in temperature when the liquid starts to boil.

Atom

Element composed of one type, the {blank}.

Nucleus

The center of a atom.

Protons

Particles in a atom with a positive charge.

Neutrons

Particles in a atom with no charge.

Electrons

Particles in a atom with a negative charge.

Electron Cloud

Area around a nucleus where electrons are mostly found.

Atomic Number

Number of protons in an atom is equal to a number called {blank}.

Mass Number

This number is the sum of the number of protons and neutrons.

Isotopes

Atoms of the same element that have different numbers of neutrons.

Average Atomic Mass

Is the weighted average mass of its isotopes.

Periodic Table

A table filled with elements in order of atomic numbers, etc.

Groups

The vertical columns in the periodic table.

Periods

Horizontal rows of elements.

Metals

Good conductors of heat and electricity.

Malleable

Can be hammered.

Ductile

Flexible.

Metallic Bonding

Positively charged metallic ions surrounded by a electron cloud.

Transitional Elements

Between groups 1 and 2, and 13 and 18.

Nonmetals

Usually gasses or brittle solids at room temperature.

Diatomic Molecule

Consists of 2 atoms of the same element in a covalent compound.

Sublimation

The process of a solid going directly into a vapor.

Metalloids

Has properties of both nonmetals and metals.

Chemical Formula

A formula that shows what elements are in a compound and what it will become.

Molecule

A neutral molecule that forms as a result of electron sharing.

Binary Compound

Composed of two elements.

charge

Tells you how many electrons an atom has gained or lost.

Polyatomic Ion

Positively or negatively charged, covalently bonded group. ( 2 or more elements that carry a charge ex OH-)

Chemical Reaction

More than one substances turning into other substances.

Reactants

Substances that react.

Products

Substances that are made.

Coeffecients

Numbers in front of each substance in a equation.

Combustion Reaction

Substance reacts with oxygen to make heat and light.

Synthesis Reaction

2 or more substances that combine to make another.

Decomposition Reaction

One substance breaks down, into 2 more.

Single Displacement Reaction

One element replaces another to make a product.

Double Displacement Reaction

Two elements replace another to make a product.

absolute zero :

The temperature at which no more energy can be removed from matter

accuracy :

how close a measurement is to the true value

Acid

A substance that increases the hydrogen ion concentration of a solution.

activation energy

the minimum amount of energy required to start a chemical reaction

chemical equation :.

A representation of a chemical reaction that uses symbols to show the relationship between the reactants and the products

chromatography :

A technique that is used to separate the components of a mixture based on the tendency of each component to travel or be drawn across the surface of another material.

collision theory

atoms, ions, and molecules can react to form products when they collide, provided that the particles have enough kinetic energy

Concentration

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

condensation :

The change of state from a gas to a liquid

conjugate acid :

an acid that forms when a base gains a proton

conjugate base :

a base that forms when an acid loses a proton

Dalton's law of partial

pressures::

Total pressure of a gas is equal to the sum of the partial pressure of the component gases

salt :

An ionic compound made from the neutralization of an acid with a base.

radioactive

elements that spontaneously emit radiation

relative formula mass

The sum of the relative atomic masses of the elements as given in the formula for any non-molecular compound.

relative atomic mass

The measure of the mass of one atom of an atom (nucleon number)

actual yield

the measured amount of a product obtained from a reaction

alkaline earth metals

the elements in Group 2A of the periodic table

alakali metals

Group 1A

Amphoteric

a substance that can act as both an acid and a base

Electronegativity

A measure of the ability of an atom in a chemical compound to attract electrons

ionization energy

The amount of energy required to remove an electron from an atom

vaporization :

The change of state from a liquid to a gas

valence electron

Electrons on the outermost energy level of an atom

Charles's Law

A principle that describes the relationship between the temperature and volume of a gas at constant pressure

cation

A positively charged ion

Bronsted-Lowry acid :.

proton donor

Arrhenius acid/base

theory:

Acids lose H+ in solution while bases lose OH- in solution

aqueous :

dissolved in water

atomic radius :

size of an atom

Boyle's Law :

:

A principle that describes the relationship between the pressure and volume of a gas at constant temperature

base :

A substance that decreases the hydrogen ion concentration in a solution.

avogadros constant

Number of molecules in 1 mole = 6.022 × 10²³

atomic mass unit (a.m.u.) :

a unit of mass equal to one-twelfth the mass of a carbon-12 atom