Chemistry Final

Front 1

calorie

Back 1

a unit of energy, the amount of energy needd to raise the temperature of 1 g of water by 1 degree celecius 1 cal = 4.184 joules

Front 2

calorimeter

Back 2

an apparatus used to measure the evolution of heat

Front 3

bomb calorimeter

Back 3

a device for measuring the heat evolved in the combustion of a substance under constant volume conditions

Front 4

bohr model of the atom

Back 4

prediction that electrons would travel in certain orbits with one orbit being its home orbit, only worked with 1 e- like H

Front 5

Dimitri Mendeleev

Back 5

father of the periodic table; predicted the existence of elements

Front 6

atomic radius

Back 6

an estimate of the size of an atom in which it has assumed to be a sphericaal object

Front 7

acid

Back 7

a substance able to donate h+ ions and then the concentrtion of H+ increases when it dissolves in water

Front 8

base

Back 8

a substance that is an h+ acceptor, produces an excess of OH which dissolved in water

Front 9

characteristics of metals

Back 9

malleable, ductile, solid at room temperature, have luster, are conductors
•Solids at room temperature (except mercury)
•High melting points
•High densities
•Large atomic radii
•Low ionization energies
•Usually, high deformation, malleable, and ductile
•Usually good thermal and electrical conductors
•Metallic lustrous appearance

Front 10

characteristics of nonmetals

Back 10

solids and not gases,
•High ionization energies
•High electronegativities
•Poor thermal conductors
•Poor electrical conductors
•Brittle solids
•Little or no metallic luster
•Gain electrons easily

Front 11

alkali metals

Back 11

member of group 1A in the periodic table

Front 12

alkaline earth metals

Back 12

members of group 2A in the periodic table

Front 13

covalent bond

Back 13

a bond formed between two or more toms by a sharing electron

Front 14

bond enthalpy

Back 14

the enthalpy changes deltaH required to break a particular bond when the substance is in gas phase

Front 15

atmospheric pressure

Back 15

a unit of pressure atm

Front 16

boyle's law

Back 16

a law stating that at a constant temperature the product of volume and pressure of a given amount of a gas is constant

Front 17

charles' law

Back 17

a law stating that at constant pressure the volume of a given quantity of gas is proportional to the absolute temeperature

Front 18

daltons law of parital pressure

Back 18

a law stating that the total pressure of a mixture of gases is the sum of the pressures that each gas would exert if it were present alone

Front 19

condensation/decomposition

Back 19

from a gas to a liquid = condensation
from a gas to a solid = decomposition

Front 20

critical temperature and pressure

Back 20

highest temperature at which it is possible to convert the gaseuos form of a substance to a liquid, pressure at which a gas is at its critical temperature and is converted to a liquid state

Front 21

alkane

Back 21

ethane c2h6 one bond

Front 22

alkene

Back 22

c2h4 double bond ethene

Front 23

alkyne

Back 23

c2h2 triple bond ethyne

Front 24

work

Back 24

the movement of an object against some force

Front 25

heat

Back 25

the flow of energy from a body of higher temperature to an area of lower when they are placed at thermal contact

Front 26

system

Back 26

thermodynamics- the portion of the universe singled out for study

Front 27

surroundings

Back 27

everything that lies outside the system we study

Front 28

first law of thermodynamics

Back 28

energy is conseved in any process a change in internal energy of a system in any process is equl stem, to the heat q, added to the system, plus any work, w, done on the system by is surroundings

Front 29

energy

Back 29

the ability to do work or tansfer heat

Front 30

exothermic

Back 30

a process in which a system releases heat to the surroundings

Front 31

endothermic

Back 31

a process in which a system absorbs heat from its surroundings

Front 32

enthalpy

Back 32

a quantity defined by the relationship h= e + pv the enthalpy change, deltaH for a reaction that occurs at constant pressure is the het evolved or absorbed in the reaction

Front 33

specific heat

Back 33

the heat capacity of 1 g of a substance, the het required to riase the temperature of 1 g of a substnce by 1 degree C

Front 34

heat capacity

Back 34

the quantity of heat required to raise the temperature of a sample of matter by 1 degree celcius

Front 35

Hess's Law

Back 35

the heat evolved in a given process can be expressed as the sum of the heats of several processes that, when added yield the process of interest

Front 36

enthalpy of formation

Back 36

the enthalpy change that accompanies the formation of substance from the most stable forms of its component elements

Front 37

standard enthalpy of formation

Back 37

the change in enthalpy that accompanies the formation of 1 mol of substance from its elemnts with all their substances in standard states

Front 38

fuel value

Back 38

the energy released when 1 g of a substance in combusted

Front 39

electromgnetic radiation

Back 39

a form of energy that has wave characteristics and that propagates through a vacuum at the characterustic speed of 3.00 x 10^8 m/s

Front 40

electromagnetic spectrum

Back 40

Radio waves, microwaves, infra red, visible light, ultra violet, x-rays, gamma rays. That was in increasing energy.

Front 41

photon

Back 41

the smallest increment of a radiant energy, a photon of light with the frequency v has an energy equal to hv

Front 42

photoelectric effect

Back 42

._________

Front 43

planck's constant

Back 43

.________

Front 44

max planck

Back 44

.______

Front 45

niels bohr

Back 45

._________

Front 46

Louis De broglie

Back 46

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