Hesi A2 Study: Chemistry

Front 1

Ionic bond.

Back 1

Relatively weak attraction between an anion and a cation. Easily disrupted in water, as when salt dissolves.

Front 2

Anion.

Back 2

A particle that gains electrons, thus acquiring a NEGATIVE charge.

Front 3

Cation.

Back 3

A particle that loses electrons, thus acquiring a POSITIVE charge.

Front 4

Covalent bond.

Back 4

Sharing of one or more pairs of electrons between nuclei.

Front 5

Single covalent.

Back 5

Sharing of one electron pair.

Front 6

Double covalent.

Back 6

Sharing of two electron pairs. Often occurs between carbon atoms, between carbon and oxygen, and between carbon and nitrogen.

Front 7

Nonpolar covalent.

Back 7

Covalent bond in which electrons are equally attracted to both nuclei. May be single or double.
STRONGEST TYPE OF CHEMICAL BOND.

Front 8

Polar covalent.

Back 8

Covalent bond in which electrons are more attracted to one nucleus than to the other, resulting in slightly positive and negative regions in one molecule. May be single or double.

Front 9

Hydrogen bond.

Back 9

Weak attraction between polarized molecules or between polarized regions of the same molecule. Important in the three-dimensional folding and coiling of large molecules. Easily disrupted by temperature and pH changes.

Front 10

Van der Waals force.

Back 10

Weak, brief attraction due to random disturbances in the electron clouds of adjacent atoms.
WEAKEST OF ALL BONDS.

Front 11

Molecular weight of a compound.

Back 11

The sum of the atomic weights of it s atoms.

Front 12

Molecule.

Back 12

Chemical particle composed of two or more atoms united by a chemical bond.

Front 13

Compound.

Back 13

Molecules composed of two or more different elements.

Front 14

Isomer.

Back 14

Molecules with identical molecular formulae but different arrangements.

Front 15

Isotope.

Back 15

Varieties of the same element that differ only in number of neutrons and therefore in atomic mass.

Front 16

Five biologically important properties of water.

Back 16

1. Solvency.
2. Adhesion.
3. Cohesion.
4. Chemical reactivity.
5. Thermal stability.

Front 17

Solvency.

Back 17

The ability to dissolve other chemicals.

Front 18

Adhesion.

Back 18

The tendency of one substance to cling to another.

Front 19

Cohesion.

Back 19

The tendency of molecules from the same substance to cling to each other.

Front 20

Chemical reactivity.

Back 20

The ability to participate in chemical reactions.

Front 21

Thermal stability.

Back 21

Result of high specific heat (the amount of heat necessary to raise the temperature of 1g of that molecule by 1º.

Front 22

Exergonic reactions.

Back 22

Reactions in which there is a net release of energy. The products have less total free energy than the reactants did.

Front 23

Oxidation.

Back 23

An exergonic reaction in which a molecule gives up electrons and releases energy. The product is then said to be oxidized.
OIL: oxidation is losing (electrons).

Front 24

Decompositon.

Back 24

An exergonic reaction, such as digestion and cell respiration, in which larger molecules are broken down into smaller ones.

Front 25

Catabolism.

Back 25

An exergonic reaction and the sum of all decomposition reactions in the body.

Front 26

Endergonic reactions.

Back 26

Reactions in which there is a net input of energy. The products have more total free energy than the reactants did.

Front 27

Reduction.

Back 27

An endergonic reaction in which a molecule gains electrons and energy. The product is then said to be reduced.
RIG: reduction is gaining (electrons).

Front 28

Reducing agent.

Back 28

A molecule that donates electrons to another.

Front 29

Atomic number.

Back 29

Is equal to the number of protons.

Front 30

Number of electrons is equal to:

Back 30

The number of protons.

Front 31

Atomic weight.

Back 31

Number of protons plus the number of neutrons.

Front 32

Atomic mass.

Back 32

The same as atomic weight, though usually rounded to nearest whole number.