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Intro to Chemistry > Unit 3 > Flashcards

Unit 3 Flashcards

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1
Q

element

A

a substance that can’t be broken down into other substances by chemical methods

microscopic form - sometimes used to mean a single atom of that element

macroscopic form - other times used to mean a sample large enough to weigh on a balance

generic form - when we say human body contains sodium, doesn’t mean elemental sodium is present, rather atoms of some form of sodium; many r soluble

118 elements, 88 of which occur naturally

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2
Q

chemical symbols

A

used as abbreviations for element names

if 3 letters = unknown

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3
Q

Al

A

Aluminum

13

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4
Q

Ar

A

Argon

18

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5
Q

Ba

A

Barium

56

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6
Q

B

A

Boron

5

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7
Q

Br

A

Bromine

35

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8
Q

Ca

A

Calcium

20

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9
Q

C

A

Carbon

6

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10
Q

Cl

A

Chlorine

17

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11
Q

Cr

A

Chromium

24

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12
Q

Co

A

Cobalt

27

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13
Q

Cu

A

Copper (cuprum)

29

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14
Q

F

A

Fluorine

9

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15
Q

Au

A

Gold (aurum)

79

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16
Q

He

A

Helium

2

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17
Q

H

A

Hydrogen

1

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18
Q

I

A

Iodine

53

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19
Q

Fe

A

Iron (ferrum)

26

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20
Q

Pb

A

Lead (plumbum)

82

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21
Q

Li

A

Lithium

3

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22
Q

Mg

A

Magnesium

12

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23
Q

Mn

A

Manganese

25

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24
Q

Hg

A

Mercury (hydrargyrum)

80

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25
Q

Ne

A

Neon

10

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26
Q

Ni

A

Nickel

28

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27
Q

N

A

Nitrogen

7

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28
Q

O

A

Oxygen

8

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29
Q

P

A

Phosphorus

15

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30
Q

Pt

A

Platinum

78

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31
Q

K

A

Potassium (kallium)

19

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32
Q

Si

A

Silicon

14

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33
Q

Ag

A

Silver (argentium)

47

34
Q

Na

A

Sodium (natrium)

11

35
Q

Sr

A

Strontium

38

36
Q

S

A

Sulfur

16

37
Q

Ti

A

Titanium

22

38
Q

Zn

A

Zinc

30

39
Q

Dalton’s Atomic Theory

A
  1. Most natural materials are mixtures of pure substances.
  2. Pure substances are either elements or compounds
  3. law of constant composition
  4. Elements are made of atoms
  5. All atoms of a given element r identical
  6. the atoms of a given element r diff from those of any other element
  7. atoms of 1 element can combine with atoms of other elements to form compounds.
40
Q

compounds

A

a distinct substance that is composed of the atoms of 2+ elements & always contains exactly the same relative masses of those elements

can be broken down into elements by chem methods

always has the same relative #’s & types of atoms

41
Q

law of constant composition

A

a given compound always contains the same proportions (by mass) of the elements.

Ex: water always contains 8g of oxygen for each gram of hydrogen

42
Q

atoms

A

tiny particles of which elements are made

indivisible in chem processes

not created/destroyed in chem reactions. reaction only changes the way the atoms r grouped together

43
Q

chemical formula

A

expresses the type of atoms & #’s of each atom in a given compound

table salt = NaCl

water = H2O

44
Q

chemical name

A

table salt = sodium chloride

45
Q

electron

A

a negatively charged particle

located outside of nucleus in a negatively charged “cloud”

most of volume of atom

46
Q

proton

A

a positively charged particle, same size of charge as an electron, but positive

47
Q

neutron

A

a neutral particle w/ a mass relatively close to that of proton

48
Q

nucleus

A

small dense center of atom

protons & neutrons

most of the mass of atom

49
Q

why do diff atoms have diff chem properties?

A

the # & arragnement of the electrons

the space in which the electrons move accounts for most of the atomic volume. the electrons r the parts of the atoms that intermingle when atoms combine to for molecules. the # of electrons a given atom possesses greatly affects the way it can interact w/ other atoms

50
Q

atomic number

A

the identity of an element is determined by this

the # of protons

51
Q

isotopes

A

(of an element)

have the same # of protons, & therefore the same atomic #, but diff #’s of neutrons

52
Q

mass number

A

the total # of protons & neutrons in an atom

used in naming to identify isotopes, such as Carbon-14 & Carbon-12

53
Q

practical purpose of isotopes

A

Iodine-123 (half-life 13 hours) is the isotope of choice for nuclear medicine imaging of the thyroid gland, which naturally accumulates all iodine isotopes

54
Q

metals

A

good conductors of heat & electricity

shiny

malleable

ductile

always form cations; tendency to lose electrons = a fundamental characteristic of metals

55
Q

shiny

A

have luster

56
Q

malleable

A

can be hammered into sheets

flattens/bends w/out shattering

57
Q

ductile

A

can be drawn into wires

58
Q

comparison of electron models

A
59
Q

nonmetals

A

good insulators

dull appearance

most r gases/easily vaporized solids & liquids

solids r brittle

60
Q

insulator

A

absorbs electricity

61
Q

metalloids

A

exhibit some prop’s of both metals & nonmetals

62
Q

groups

A

all elements in a group have similar chem prop’s

63
Q

Group 1

A

Alkali Metals

64
Q

Group 2

A

Alkaline Earth Metals

65
Q

Groups 3-12

A

Transition Metals

66
Q

Group 17

A

Halogens

67
Q

Group 18

A

Noble Gases

68
Q

diatomic molecules

A

cannot stand alone

2 atoms

hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine

HINClBrOF

69
Q

ions

A

the equal # of protons & electrons gives an atom a net zero charge

adding or removing an electron from a neutral atom will create a charged ion

always fromed by adding/removing electrons, not by changing the # of protons

70
Q

cation

A

positive ion

when atom loses 1+ electrons

Na → Na+ + e-

named using name of the parent atom

Ex: Na+ is called the sodium ion

71
Q

anion

A

negative ion

when an atom gains 1+ electrons

Cl + e- → Cl-

named by taking the root name of the atom & changing the ending (adding -ide)

72
Q

common anion name changes

A

chlorine - chloride ion

flourine - flouride

bromine - bromide

iodine - iodide

oxygen + 2 electrons = oxide

sulfur + 2 electrons = sulfide

73
Q

ion group charges

A

Group 1 metals - +1

Group 2 metals - +2

many Group 3-12 metals - multiple charges

Group 13 metals - +3

Group 16 atoms - -2

Group 17 atoms - -1

74
Q

ionic compounds

A

whenever a compound is formed b/w a metal & non-metal, it can be expected to contain ions

usually formed when metals + nonmetals; when they react, the metal atoms tend to lose 1+ electrons, which r gained by the atoms of the nonmetals; the reactions tend to form compounds that contain metal cations & nonmetal anions

chem compounds must have net charge of 0 - must be cations & anions present; the # of cations & anions must result in net charge of zero

usually strong electrolytes & can be expected to dissociate completely in solution

75
Q

rules for compound formula writing

A

the cation/metal/pos. is always written first

use subscripts to balance charges on compounds

76
Q

brittle

A

shatters/cracks into small pieces when struck

77
Q

strong electrolyte

A

a substance that separates into ions when dissolved in water

78
Q

dissociation

A

the process in which ionic compounds separate into ions

79
Q

molecular compounds

A

usually non-electrolytes & don’t dissociate to form ions

resulting solutions don’t conduct electricity

80
Q

molecular acids

A

can partially/completely dissociate, depending on their strength

81
Q

W

A

tungsten

74

Intro to Chemistry (6 decks)

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