Glossary of Terms

How close a measured value is to the accepted or real value.

The amount of products actually formed during a chemical reaction.

Electric current equal to one coulomb per second.

The shape of an orbital.

0,1,2,3,…,n-1

Each value for l is a subshell

Each number value of l is assigned a letter s,p,d,f,g….

When:
n=1, l=0: 1s
n=2, l=0,1: 2s,2p

Elements that have unpredictable properties.
A main group NONMETAL will GAIN electrons to form an ANION with the same number of electrons as the nearest noble gas.

Elements that have unpredictable properties.
A main group NONMETAL will GAIN electrons to form an ANION with the same number of electrons as the nearest noble gas.

A substance that produces H⁺ in an aqueous solution, strong acids completely dissociate in aqueous solution.

A substance in an aqueous solution that produces OH⁻, strong bases completely dissociate in aqueous solution.

Is the weighted average of isotopic masses based on the natural abundance of each isotope.

The number of protons in the nucleus of an atom. The type of atom/element is determined by the number of protons.

Electrons occupy lower energy orbitals before filling higher energy orbitals.

One or more atoms that has lost an electron(s).

A main group METAL will LOSE electrons to form a CATION with the same number of electrons as the nearest noble gas.

Electrons and protons have charge that is equal and opposite, because of this we can say the relative charge in atomic units is one.

A one or two letter abbreviation assigned to each element.

Electrons in a filled inner shell.

A ratio of mass (m) to volume (V) of a substance.

A negatively charged particle located in the volume of space surrounding the nucleus of an atom.

A notation that represents the orbitals occupied by electrons in an atom.

Write the value of n, followed by the number of electrons allowed in each orbital until all electrons in the atom are assigned to an orbital.

Example Carbon: 6 electrons = 1s²2s²2p²

One or more atoms of the same type.

A number with an unlimited amount of significant figures.

Electrons will singly occupy degenerate orbitals until they are half full before pairing up with other electrons. Electrons in half full orbitals will have the same spin.

The ion formed when a proton associates with water to form H₃O.

The OH⁻ ion.

A substance that does not readily dissolve in water.

Ions are represented as the chemical symbol of the ion with the charge of the ion noted as a superscript to the right.

Xᶜʰᵃʳᵍᵉ

Lithium ion = Li⁺, Oxygen ion = O2⁻

One or more atoms that has gained or lost an electron(s).

Ions are charged particles.

See also, Cation(+) and Anion(-)

The absolute temperature scale, 0K is assigned to absolute zero, the temperature at which all molecular motion stops

The measurement the mass of an object, how much matter it contains. Defined by a metal cylinder housed at the International Bureau of Weights and Measures in Sevres France.

Orientation of orbital in 3D space.

Value= integer values from –l…l.

There are 2(l)+1 values of ml

for each value of l.

Examples:
When:
l=0, ml= 0
l=1, ml = -1,0,1
2(0)+1=1 value of ml
2(1)+1=3 values ml

The sum of the number of neutrons and protons in the nucleus of an atom.

A numeric quantity in which every digit, except the last, is certain. The last digit is estimated, leading to an uncertainty in the measurement.

The distance light travels through a vacuum in 1/299792458s

Is defined as 6.022x10²³ objects.

Two or more bonded atoms of different types.

Two or more bonded atoms of the same type.

Two or more bonded atoms.

A neutral particle located in the nucleus of an atom.

The small dense core of an atom consisting of neutrons and protons. Neutrons and protons have approximately the same mass.

Gains electrons, is the oxidizing agent.

No two electrons in an atom can have the same four quantum numbers. But.. Any three quantum numbers can be the same.

This implies: One orbital may contain two electrons of opposite spin orientation!

Actual products formed as a percentage of the theoretical yield.
Percent Yield = (Actual Yield/Theoretical Yield) x 100

The degree of reproducibility of a measured quantity; how close a series of measurements of the same quantity are to one other.

Orbital’s size and energy level of an electron.

A whole number 1,2,3,4…..

n increases with an electron’s energy and distance from the nucleus.

Each level is called a shell.

Materials produced in a chemical reaction
2H₂+0₂ →2H₂O

A positively charged particle located in the nucleus of an atom.

Two or more molecules or atoms of the same type.

Materials consumed in a chemical reaction.
2H₂+0₂ →2H₂O

The notation used to illustrate a chemical reaction.
2H₂+0₂ →2H₂O

Loses electrons is the reducing agent.

The gain of electrons.

The duration of 9,192,631,770 periods of the radiation emitted from a transition in a cesium-133 atom.

The number of non-place holding digits in a reported measurement. A larger amount of significant figures means a larger precision in the measurement.

The maximum amount of solute that can dissolve in a solvent at a given temperature.

A substance that readily dissolves in water to a significant extent.

Material present in a solution that has a smaller molar amount.

A homogenous mixture of two or more substances consisting of ions or molecules.

Material present in a solution that has the larger molar amount.

Spin is intrinsic to all electrons, it is quantized, with only two orientations; spin up or spin down.

Value =+12 OR −12

The state that each of the products and reactants are in during the reaction; (s)-solid, (l)-liquid, (g)-gas, (aq)-aqueous.
2H₂(g)+0₂(g)→2H₂O(g)

The amount of products formed in a chemical reaction based on stoichiometric calculations.

Electrons in the outermost shell (highest n value).

Example Carbon:
6 electrons = 1s²Core

2s²2p²Valence

A unit of length raised to the third power, volume is a measure of space.