Ch1+2

Question 1

macroscopic

Answer 1

ordinary sized objects (macro=large)

Question 2

microscopic

Answer 2

atoms and molecules

Question 3

states matter

Answer 3

gas/vapor (no fixed volume or shape, molecules far apart and high speed), liquid (distinct volume but no shape), and solid (definite shape and volume, molecules tight together with little movement)

Question 4

pure substances

Answer 4

(Substances) have distinct properties and composition that doesn’t vary from sample to sample (water, salt)

Question 5

het mixtures

Answer 5

don’t have same composition, properties, and appearance throughout (rocks, wood)

Question 6

law of constant composition

Answer 6

the elemental composition of a pure compound is always the same

Question 7

phys properties

Answer 7

can be measured without changing the identity and composition of the substance (color, odor, density, melting/boiling point, hardness)

Question 8

chem properties

Answer 8

describe the way a substance may change/react to form other substances (flammability)

Question 9

intensive props

Answer 9

do not depend on the amount of the sample examined (temperature, melting point, density)

Question 10

extensive props

Answer 10

depend on the quantity of the sample (mass, volume)

Question 11

filtration

Answer 11

a mixture of a solid+liquid is poured through porous medium (filter paper) to separate solid from liquid

Question 12

distillation

Answer 12

boiling a mixture to separate into solid and gas

Question 13

Giga G

Answer 13

9

Question 14

mega M

Answer 14

6

Question 15

kilo k

Answer 15

3

Question 16

deci d

Answer 16

-1

Question 17

centi c

Answer 17

-2

Question 18

milli m

Answer 18

-3

Question 19

micro mew

Answer 19

-6

Question 20

nano n

Answer 20

-9

Question 21

pico p

Answer 21

-12

Question 22

femto f

Answer 22

-15

Question 23

C to K

Answer 23

K=ºC+273.15

Question 24

C to F

Answer 24

ºF=9/5(ºC)+32

Question 25

F to C

Answer 25

C=5/9(F-32)

Question 26

density formula

Answer 26

D=m/v.

Question 27

daltons atomic theory

Answer 27

1. ) Each element is composed of extremely small particles called atoms
2. ) Atoms of an element are identical to one another in mass and other properties but the atoms of one element are different from those of other elements
3. ) Atoms of an element are not changed into atoms of a different element by chemical reactions; atoms are neither created nor destroyed in chem reactions
4. ) Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms

Question 28

law of constant composition

Answer 28

in a given compound, the relative numbers and kinds of atoms are constant

Question 29

law of conservation of matter

Answer 29

the total mass of materials present after a chemical reaction is the same as the total mass present before the reaction

Question 30

law of multiple proportion

Answer 30

if two elements A and B combine to form more than one compound, the masses of B that can combine with the given mass of A are in the ratio of smallest whole numbers

Question 31

cathode rays

Answer 31

(mid-1800s) Scientists first studied cathode rays, radiation originated from the electrons, by applying an electric current to a chamber almost empty of air. When the voltage was applied, the rays shoot from negative plate through positive plate and cause glass to give off light. JJ Thomson uses this to “discover” the electron
Thomson used a fluorescent screen at the end of a cathode-ray tube to calculate the electron’s charge to mass quantity, 1.76* 10^8 C/g (coulombs, SI unit for charge).

Question 32

radiation

Answer 32

alpha (a), beta(b), and gamma(y). a particles have a charge of 2+ and are attracted to negative plate. b particles have a charge of 1- and are attracted to positive plate. y rays don’t consist of particles and carry no charge, so are not deflected/scattered by electric fields

Question 33

angstrom

Answer 33

Å = 10^-10m. Atoms have diameters of 1-5 Å or 100-500pm

Question 34

isotope notation

Answer 34

6(down)12(up)C(read carbon-12) has 6 protons and 6 neutrons. The subscript, 6, is the atomic number. The superscript, 12, is the mass number, the number of protons+neutrons

Question 35

atomic weights, amu

Answer 35

1 amu = 1.6605410^-24g and 1g= 6.0221410^23 amu
12 amu = 1 g of carbon-12
To calculate average atomic mass of element, you need to know masses of isotopes and their decimal abundances. (abundance isotope 1)(mass isotope 1) +(abundance isotope 2)(mass isotope 2)= avg atomic mass/atomic weight

Question 36

organic chemistry

Answer 36

Organic chemistry is the study of compounds of carbon

Organic compounds contain C and H, usually in combo with O, N or S. All other compounds are inorganic compounds.

Question 37

hydrocarbons

Answer 37

compounds that contain only carbon and hydrogen

Question 38

alkanes

Answer 38

where each C atom is bonded to four other atoms. 3 simplest alkanes: methane (CH4), ethane (C2H6), and propane (C3H8)

Question 39

alcohol

Answer 39

btained by replacing an H atom of alkane with an –OH group and the name is made by adding an -ol ending (CH3OH=methanol)
1-propanol indicates that the replacement of H with OH has occurred at one of the “outer” C atoms rather than the “middle” C atom. 2-propanol (aka isopropyl alcohol) is obtained if the OH functional group is attached to the middle carbon atom

Question 40

naming acids

Answer 40

• ide=hydro_ic
• ate=-ic
• ite=-ous

Question 41

mass spectrometer

Answer 41

measures mass of atom

Question 42

cathode ray tube

Answer 42

discovered electron (thomson)

Question 43

oil drop

Answer 43

discovered charge of e (millikan)