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General Chemistry > Chapter 2 vocab > Flashcards

Chapter 2 vocab Flashcards

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1
Q

What did dalton do

A

bring back the idea of the atom. created “Daltons Atomic Theory” based on 3 laws

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2
Q

what are the 3 laws dalton based his theory on

A

law of constant composition
law of conservation of mass
law of multiple proportions

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3
Q

what does the law of constant composition mean

A

that there is the same number of atoms in any sample. every grain of salt is NaCl. discovered by joseph proust

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4
Q

what does the law of conservation of mass mean

A

the total mass of substances present at the end of a chemical process is the same as the mass in the beginning

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5
Q

what is the law of multiple proportions

A

if i make a new compound I can only add or subract by a whole atom, not half at atom

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6
Q

4 postulates of daltoms atomic theory

A
  1. each element is composed of small particles called atoms
  2. all atoms of a given element are identical, but the atoms of one element can differ from t he atoms of other elements
  3. atoms of one eleemtn cant be changed into atoms of a diff eleement by chemical reactions, elements cant be created or destroyed
  4. compounds are formed when atoms of more than one element combine
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7
Q

who tested the electon? and what?

A

JJ thomson used cathode rays to discover charge to mass ratio of 1.76E^8 coulombs/gram
millikan disovered charge and mass of an electron (the oil drop)

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8
Q

what is radioactivity

A

spontaneous emission of high radiation by an atom

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9
Q

who studied radioactivity

A

marie and pierre curie. and henri becquerel observed it

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10
Q

what did radioactivity prove

A

led to a discovery that an atom had subatomic particles and energy

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11
Q

Three types of radiation?

A

a` positive
a ^ negative
a~ no charge

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12
Q

how was the nucleas discovred

A

shot positive particles at a thin sheet of gold foil to observe the pattern of the particles

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13
Q

What is most of an atom?

A

empty space

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14
Q

what is in a nucleus

A

protons and neutrons

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15
Q

Proton mass

A

1.0073 amu

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16
Q

Nuetron mass

A

1.0087 amu

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17
Q

Electron mass

A

close to 0 (5.486E^-4 amu)

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18
Q

What is an atomic number

A

the number of protons in the nucleus

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19
Q

top left of an element symbol resembles what

A

the mass number

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20
Q

bottom left of an element symbol resemles what

A

the atomic number

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21
Q

how to get mass #

A

protons AND neutrons

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22
Q

how to get atomic #

A

protons OR electrons

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23
Q

What does isotope mean

A

atoms of the same element with different masses, meaning different # of neutrons

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24
Q

Amu means?

A

Atomic mass unit

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25
Q

1 amu =

A

1.66054 E^-24 g

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26
Q

Atomic weight =
(equation)

A

sum of ( (isotope mass) x ( fractional natural abundance) )

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27
Q

Periodic table row?

A

periods

28
Q

periodic table column ?

A

groups

29
Q

Metals ?

A

on left

30
Q

elements in same what have similar chemical properties?

A

groups/ columns

31
Q

nonmetals?

A

on right

32
Q

metalloids ?

A

diagonal middle line

33
Q

1A is

A

alkali metals

34
Q

2A is

A

Alkaline earth metals

35
Q

6A is

A

Chalogens

36
Q

7A is

A

Halogens

37
Q

8A is

A

Noble gases

38
Q

Periodicity def

A

repeating pattern of properties and reactivity

39
Q

metals traits

A

shiny
left side (besides H)
conduct heat and electricity
solids (besides Mercury)

40
Q

Non metals traits

A

right side (and H)
solid, liquid or gas at room temp

41
Q

metalloids traits

A

sometimes like metal, sometimes like nonmetals
steplike line

42
Q

Chemical formula ? for water

A

H2O

43
Q

Molecular compounds ?

A

with molecules. almost always contain only nonmetals

44
Q

Diatomic molecules. name the 7

A

Hydrogen
Nitrogen
Oxygen
Fluorine
Chlorine
Bromine
Iodnine

45
Q

2 types of formulas

A

empirical or molecular

46
Q

Empirical formula def

A

gives the lowest whole number ration of atoms of each element in a compound

47
Q

molecular formulas def

A

give the exact number of atoms of each element in a compound

48
Q

can you go from empirical to molecular?

A

no

49
Q

structural formulas

A

they show the order in which atoms are attached. not 3 D

50
Q

what can be used to show a 3d model of atoms

A

perspective drawings, ball and stick models, and space filing models

51
Q

Positively charged ion

A

cation

52
Q

negatively charged ion

A

anion

53
Q

Ions def

A

when an atom of a group of atoms loses or gains electrons, it becomes an ion

54
Q

Cation means what about the atom

A

it lost at least one electron, Monatomic are formed by metals

55
Q

ANion means what about the atom

A

it gained at least one electron, monatomic are formed by nonmetals, execpt the noble gases

56
Q

Octel rule ?

A

Atoms try to reach a number equal with group 8A . the nobel gases

57
Q

Monoatomic vs Polyatomic ions

A

Poly means a group of atoms

58
Q

what is NH4 +

A

a polyatomic cation

59
Q

what is SO4 2-

A

a polyatomic anion

60
Q

Ionic compund def

A

generally formed between metal snad nonmetals. electrongs go from metal to nonmetal. only writen in empirical formulas.

61
Q

Mg +2 paired with N -3

A

Mg3N2

62
Q

Inorganic Nomenclature writing means a polyatomic cation will end in what ?

A

write name as is if regular cation
ium for polyatomic

63
Q

Inorganic Nomenclature writing means a anion will end in what ? what about a polyatomic anion?

A

ide for regular anion
write name as is if polyatomic

64
Q

(NH4)2SO4

A

Ammonium Sulfate

65
Q

FeCl

A

Iron (II) Chloride

66
Q

NaCl

A

Sodium Chloride

67
Q

Fe3(PO4)2

A

Iron (II) Phosphate

General Chemistry (9 decks)

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