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Chemistry 107 > Chapter 2 - Atoms, Ions, Molecules > Flashcards

Chapter 2 - Atoms, Ions, Molecules Flashcards

0
Q

Atomic Symbol

A

Used to represent an atom corresponding to a particular element

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1
Q

Dalton’s Atomic Theory

A
  1. Each element is composed of tiny, indestructible particles called atoms
  2. All atoms of a given element have the same mass and other properties that distinguish them from atoms of other elements
  3. Atoms combine simple, whole-number ratios to form molecules of compounds
  4. In a chemical reaction, atoms of one element cannot change into atoms of another element. They simply rearrange the way they are attached
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2
Q

Subatomic Particles of Atoms and their Charges

A

Protons(+)
Electrons(-)
Neutrons(neutral)

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3
Q

Rutherford’s Model of Atomic Structures

A

Atom = dense, heavy nucleus at center
Nucleus contains protons and neutrons (both make up nearly entire mass of atom)
Nucleus surrounded by electron cloud

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4
Q

JJ Thomson (1856-1940)

A

Discovered electrons in 1897 using a cathode-ray tube

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5
Q

Cathode-Ray Tube

A

Consists of glass tube where most if the air was removed.

Used by JJ Thomson to discover electrons

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6
Q

Plum Pudding Model (of atom)

A

Idea of a positively charged nucleus and the negatively charged electrons distributed throughout the positively charged sphere

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7
Q

Robert Millikan (1868-1953)

A

Determines the charge of electron through oil drop experiment

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8
Q

Henri Becquerel (1896)

A

Discovered radioactivity

Noticed that some materials produced invisible radiation consisting of charged particles

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9
Q

Radioactivity

A

Spontaneous emission of high energy radiation particles (beta, alpha particles)

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10
Q

Beta Particles (B)

A

High energy electrons (negatively charged)

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11
Q

Alpha Particles (a)

A 
Positively charged (+2)
Mass= He nucleus
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12
Q

Atomic Mass Unit (amu)

A

Unit used to express relative masses of atoms and subatomic particles
1amu = 1/12 of carbon atom
(Carbon made up of 6protons 6neutrons)
1amu = 1 Dalton (Da)

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13
Q

Dalton (Da)

A

1 Da = 1 amu

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14
Q

Francis W. Aston (1877-1945)

A

Used charged beam of neon (Ne+) and noticed 2 signals which meant 2 different isotopes
Discovered isotopes

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15
Q

Isotopes

A

Atoms of an element containing the same number of protons but different neurons
Ex. neon
1 isotope has 10 neutrons in it’s nucleus and a mass of 20amu
Another isotope has 12 neutrons and a mass of 22amu (protons remain the same)

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16
Q

Nuclides

A

Each individual isotope with a particular combo of protons and neutrons

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17
Q

Atomic Number

A

Number of protons in the nucleus

Determines identity of element

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18
Q

Atomic Mass Number

A

Total number of nucleons (protons & neutrons) in nucleus

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19
Q

Average Atomic Mass

A

Weighted average of masses of all isotopes of an element

Calculated by multiplying natural abundance by its mass (im amu) and then summing these products

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20
Q

Natural Abundance

A

Proportion of a particular isotope; usually expressed as a percentage relative to all isotopes for that element
(How much of each isotope exists in relative to the other isotopes existing for that element)
Only non-decaying stable isotopes occur naturally and therefore have natural abundance

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21
Q

Dimitri Mendeleev (1834-1907)

A

1872 - published a periodic table
Ordered elements by increasing atomic mass (in modern: ordered by atomic numbers)
Arranged elements in columns based on similar chemical & physical properties
Left open spaces for elements not yet discovered
Based on the locations of the empty cells he was able to predict the chemical and physical properties

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22
Q

Modern Period Table

A

Elements classified according to physical and chemical properties (like Mendeleev)
Horizontal Rows= periods (1-7)
Columns= groups- contain elements of the same family (or group) (1-18)

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23
Q

Alkali Metal

A

Group 1
Have 1 valence electron (want to lose electron)
Shiny, soft metals, highly reactive
Do not occur naturally as free elements
Reactivity increases down the group(as outer electron gets further from nucleus and becomes easier to remove)
By losing electron they become cation and stable

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24
Q

Alkaline Earth Metal

A

Group 2
2 valence electrons

Harder, denser, stronger than alkali
Have higher melting points than alkali
Lower reactivity than alkali
React with water to form metal hydroxides

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25
Q

Anion

A

Negatively charged particle created when an atom or molecule gains one or more electrons

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26
Q

Cation

A

Positively charged particle created when an atom or molecule loses one or more electrons

27
Q

Carboxylic acid

A

Organic compound containing -COOH functional group

28
Q

Covalent Bond

A

A bond between two atoms created by SHARING one or more electrons

2 nonmetals

29
Q

Law of Multiple Proportions

A

The ratio of the two masses of one element react with a given mass of another element to form two different compounds is the ratio of two small numbers

30
Q

Molecular Compound

A

Composed of atoms held together in molecules by covalent bonds (nonmetals)

31
Q

Molecular Formula

A

Shows the # and type of atoms present in one molecule of a compound

32
Q

Empirical Formula

A

Shows the smallest whole number ratio of elements in a compounds

33
Q

Ionic Compounds

A

Consist of charged particles (ions) formed by transfer of electrons between atoms
(Between metals and nonmetals)

34
Q

CH3COO-

35
Q

NH4+

36
Q

N3-

37
Q

Br-

38
Q

CO3 2-

39
Q

ClO3-

40
Q

Cl-

41
Q

CrO4 2-

42
Q

CN-

43
Q

Cr2O7 2-

A

Dichromate

44
Q

H2PO4-

A

Dihydrogen Phosphate

45
Q

S2 2-

46
Q

F-

47
Q

H-

48
Q

HCO3-

A

Hydrogen Carbonate
or
Bicarbonate

49
Q

HPO4 2-

A

Hydrogen Phosphate

50
Q

HSO3-

A

Hydrogen sulfite or bisulfite

51
Q

OH-

52
Q

NO3-

53
Q

N 3-

54
Q

NO2-

55
Q

O2-

56
Q

ClO4-

A

Perchlorate

57
Q

MnO4-

A

Permanganate

58
Q

O2 2-

59
Q

PO4 3-

60
Q

SO4 2-

61
Q

S2 -

62
Q

SO3 2-

63
Q

SCN-

A

Thiocyanate

64
Q

Naming Binary MOLECULAR Compounds

A

(contain 2 nonmetals)

  1. Name first element
  2. Change ending of name of second element to -ide
  3. Add prefixes to first & second names to indicate # of atoms (do not use mono on first element)
65
Q

Naming Binary IONIC Compounds

A

(Contain cations (metals) & anions (nonmetals))

  1. Name metal (cation)
  2. Name nonmetal (anion) with ending changed to ide

Transition metals - use roman numeral to indicate charge

66
Q

Naming Binary ACIDS

A
  1. Add prefix hydro-

2. Replace last syllable in name with suffix -ic & add acid at the end

Chemistry 107 (4 decks)

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