General

Question 1

Mass Number

Answer 1

the total number of protons and neutrons in a nucleus

Question 2

Atomic Number

Answer 2

the number of protons in the nucleus of an atom, which determines the chemical properties of an element and its place in the periodic table

Question 3

Proton

Answer 3

a stable subatomic particle occurring in all atomic nuclei, with a positive electric charge equal in magnitude to that of an electron, but of opposite sign

Question 4

Neutron

Answer 4

a subatomic particle of about the same mass as a proton but without an electric charge, present in all atomic nuclei except those of ordinary hydrogen

Question 5

Electron

Answer 5

a stable subatomic particle with a charge of negative electricity, found in all atoms and acting as the primary carrier of electricity in solids

Question 6

Isotope

Answer 6

each of two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei, and hence differ in relative atomic mass but not in chemical properties; in particular, a radioactive form of an element

Question 7

Atom

Answer 7

the basic unit of a chemical element

Question 8

Atomic Weight

Answer 8

The average mass of atoms of an element, calculated using the relative abundance of isotopes in a naturally-occurring element. It is the weighted average of the masses of naturally-occurring isotopes

Question 9

Elements in the same column

Answer 9

group or family

Question 10

Alkali Metals

Answer 10

Column A1

Question 11

Alkaline Earth Metals

Answer 11

Column A2

Question 12

Halogens/Halides

Answer 12

Column A7

Question 13

Noble Gasses

Answer 13

Column A8

Question 14

Transition Metals

Answer 14

Columns B1-B10

Question 15

Electron Shell

Answer 15

a grouping of electrons surrounding the nucleus of an atom

Question 16

Valence Electron

Answer 16

an electron in the outer shell of an atom which can combine with other atoms to form molecules

Question 17

Valence Shell

Answer 17

the outermost shell of electrons in an atom; these electrons take part in bonding with other atoms

Question 18

Core Shells

Answer 18

the shells of electrons within the valence shell

Question 19

Nuclear Radiation

Answer 19

the process by which a nucleus of an unstable atom loses energy by emitting particles of ionizing radiation

Question 20

Alpha Radiation

Answer 20

loss of 2 protons and 2 neutrons; ionizing radiation consisting of alpha particles, emitted by some substances undergoing radioactive decay;

Question 21

Beta Radiation

Answer 21

loss of an electron and gain of a proton; radiation of beta particles during radioactive decay

Question 22

Gama Radiation

Answer 22

emition of high energy light;

Question 23

Half Life

Answer 23

the time taken for the radioactivity of a specified isotope to fall to half its original value

Question 24

Octet Rule

Answer 24

each atom attempts to achieve 8 valence electrons with the exception of hydrogen, boron, and aluminum;

Question 25

Ionic Bond

Answer 25

a chemical bond formed between two elements when the difference in their electronegativity is greater than 1.7; a chemical bond in which one atom loses an electron to form a positive ion and the other atom gains an electron to form a negative ion; bonds formed primarily between elements from either side of the metaloid line; elements to the right gain one or more electrons and form anions with a negative charge; elements on the left lose one or more electrons to form cations with a positive charge; bonds between a metal and non-metal are ionic;

Question 26

Covalent Bond

Answer 26

a chemical bond that involves sharing a pair of electrons between atoms in a molecule; bonds primarily between atoms on the same side of the metaliod line;

Question 27

Salts

Answer 27

ionic compounds; compounds consisting of catons and anions through ionic bonds; usually disolve in water;

Question 28

Single Bond; Double (Diative) Bond; Tripple Bond

Answer 28

a single covalent bond consisting of one set of electrons or one electron from each element; a pair of covalent bonds consisting of two sets of electrons or two electrons from each element; a triad of covalent bonds consisting of three sets of electrons or three electrons from each element;

Question 29

Polar Covalent Bond

Answer 29

a bond formed between elements when the difference of their electronegativity is between 0.3 and 1.7; a separation of electric charge leading to a molecule or its chemical groups having an electric dipole or multipole moment; these molecules interact through dipole–dipole intermolecular forces and hydrogen bonds; it is dependent on the difference in electronegativity between atoms in a compound and the asymmetry of the compound’s structure; it underlies a number of physical properties including surface tension, solubility, and melting- and boiling-points;

Question 30

Electronegativity

Answer 30

the tendency of an atom or radical to attract electrons in the formation of an ionic bond; flourine has the highest tendancy to atract an ionic bond; the closer an element is to flourine the higher it’s tendancy towards attracting an ionic bond is; the element with the higher tendancy has a slightly negative charge;

Question 31

Non-Polar Covalent Bonds

Answer 31

bonds formed through the same element or between carbon and hydrogen;bonds between two elements when the difference of thier electronegativety is less than 0.3

Question 32

Naming Ionic Compounds

Answer 32

name of cation - root of anion, add “ide”

NaCl is sodium - chlor - ide

MgI₂ is magnesium - iod - ide

Question 33

Physical States

Answer 33

solid _(s) liquid _(l) gass _(g) aqueous _(aq) (disolved in water)

Question 34

A Balanced Equation

Answer 34

the expression of the ratio of molecules;

Question 35

Molecular Measurement

Answer 35

number of molecules by weight based on the total atomic weight of avagadros number of each of the elements in the molecule;

Question 36

Avagadro’s Number

Answer 36

6x10²³