Chem Midterm

Front 1

mass

Back 1

a measure of the amount of matter that an object contains

Front 2

weight

Back 2

a force that measures the pull of gravity on a given mass

Front 3

solid

Back 3

definite shape and definite volume

Front 4

liquid

Back 4

definite volume and take the shape of the container

Front 5

gas

Back 5

no definite volume and no definite shape

Front 6

kinetic molecular theory/ideal gas law

Back 6

a theory explaining the states of matter, based on the concept that all matter consists of tiny particles that are in constant motion

Front 7

physical change

Back 7

a change in appearance, but the substance itself is not changed

Front 8

chemical change

Back 8

a change produces a new substance with different properties

Front 9

mixture

Back 9

two or more substances are mixed together

Front 10

distillation

Back 10

process that separates dissolved solids from a liquid, which is boiled to produce a vapor that is then condensed into a liquid

Front 11

evaporation

Back 11

a conversion of a liquid to a gas that is not boiling

Front 12

filtration

Back 12

a process that separates the solid and liquid (filter paper)

Front 13

element

Back 13

a substance which cannot be decomposed into anything simpler by a chemical change

Front 14

compound

Back 14

two or more different elements

Front 15

potential energy

Back 15

stored energy

Front 16

kinetic energy

Back 16

energy of motion

Front 17

law of conservation of matter and energy

Back 17

nothing can be destroyed; only transformed

Front 18

heat

Back 18

energy that transfers from one object to another because of a temperature difference between the objects

Front 19

endothermic

Back 19

energy is absorbed

Front 20

exothermic

Back 20

energy is released

Front 21

temperature

Back 21

a measure of the average kinetic energy of the molecules

Front 22

boiling point

Back 22

when the vapor pressure equals the atmospheric pressure above the liquid

Front 23

normal boiling point

Back 23

when the vapor pressure of the liquid equals standard pressure

Front 24

melting point

Back 24

the temperature at which a substance changes from a solid to a liquid

Front 25

sublimation

Back 25

the process in which a solid changes to a gas or vapor without passing through the liquid state

Front 26

heat of fusion

Back 26

the heat needed to melt 1 gram of ice

Front 27

heat of vaporization

Back 27

the heat needed to change 1 gram of water to steam

Front 28

specific heat capacity

Back 28

amount of heat needed to raise 1 gram of water 1C

Front 29

democritus' atomic theory

Back 29

atoms were indivisible and indestructible

Front 30

nucleus

Back 30

positive center of the atom

Front 31

electrons

Back 31

negatively charged particles outside the nucleus on the shells

Front 32

atomic number

Back 32

the number of protons in the nucleus

Front 33

valence electrons

Back 33

electrons located on the outermost electron shell

Front 34

atomic mass

Back 34

measure of the weighted average of the most abundant allotropes

Front 35

AMU

Back 35

a unit of mass equal to 1/12 the mass of a carbon-12 atom

Front 36

isotope

Back 36

an atom with the same number of protons but different numbers of neutrons

Front 37

ground state

Back 37

when an atom’s electrons are where they’re supposed to be on the 1st level

Front 38

excited atom

Back 38

when the electrons absorb more energy and jump to a higher energy level

Front 39

ion

Back 39

charged atom that is produced by gaining or losing electrons from the valence shell

Front 40

isoelectronic

Back 40

two or more elements that have the same electron configuration

Front 41

metal

Back 41

elements to the left of the zigzag line

Front 42

nonmetal

Back 42

elements to the right of the zigzag line

Front 43

metalloids

Back 43

elements touching the zigzag line EXCEPT aluminum (Al)

Front 44

allotropes

Back 44

forms of the same element that have different molecular formulas or different crystalline structures

Front 45

nuclear pull

Back 45

attraction from the nucleus to the valence electrons

Front 46

ionization energy

Back 46

energy needed to remove one electron

Front 47

electronegativity

Back 47

the attraction for electrons

Front 48

atomic radius

Back 48

the distance from the nucleus to the outer valence electron

Front 49

chemical bond

Back 49

the simultaneous attraction of 2 or more nuclei for valence electrons

Front 50

ionic bond

Back 50

bond formed by the transfer of electrons

Front 51

covalent bond

Back 51

bond formed by the sharing of electrons

Front 52

polar covalent bond

Back 52

unequal sharing

Front 53

nonpolar covalent bond

Back 53

equal sharing (END: 0)

Front 54

coordinate covalent bond

Back 54

bond formed when one atom donates both electrons that are shared

Front 55

molecule

Back 55

the smallest discrete particle of an element or compound that has covalent bonds between atoms

Front 56

network solid

Back 56

atom to atoms covalently bonded forming a macromolecule with no discrete particles

Front 57

metallic bond

Back 57

positive ions surrounded by a sea of mobile elctrons

Front 58

diatomic molecule

Back 58

molecule consisting of 2 atoms

Front 59

symmetrical

Back 59

if something is folded in half both sides would be equal

Front 60

asymmetrical

Back 60

unequal distribution of charges which leads to partial charges

Front 61

dipole

Back 61

molecule with charge distributed unevenly, one end is more positive and one end is more negative

Front 62

hydrogen bond

Back 62

attractive forces in which a hydrogen atom covalently bonds to a very electronegative atom with a small atomic radius

Front 63

empirical formula

Back 63

reduced formula

Front 64

skeleton formula

Back 64

unbalance formula