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DATCrusher Chem Videos > Chemistry Video 3 > Flashcards

Chemistry Video 3 Flashcards

1
Q

Atomic Theory

A

John Dalton, 1807

  1. Matter consists of tiny particles called atoms, which are the smallest indivisible unit of a particular element
  2. An element consists of only one type of atom, which has a particular mass characteristic of that element
  3. Atoms of a given element are different from atoms of any other element
  4. A compound consists of atoms of 2 or more elements combined in whole number ratios, and that ratio is constant for that compound
  5. When a chemical change occurs, atoms are neither created nor destroyed, they simply rearrange to form different combinations
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2
Q

Law of definite proportions/Law of constant composition

A

Any sample of a compound contains the same ratio of elements by mass

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3
Q

Law of multiple proportions

A

When 2 elements react with one another, the second element can react in small whole number ratios

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4
Q

Cathode Ray Tube

A

1897, JJ Thompson. Used cathode ray tubes, which are tubes containing metal electrodes in a vacuum. When a voltage was applied, a cathode ray beam appeared between the electrodes. The cathode ray beam bends towards the positively charged plate. This indicated that inside an atom, there must be negatively charged particles. Thompson used the angle of the beam and the power of the magnetic field to calculate the charge to mass ratio of the electron and discovered that electrons are lighter than atoms. He concluded that electrons are inside atoms

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5
Q

Oil Drop Experiment

A

1909, Robert Millikan. Movement of microscopic oil droplets were studied to determine the magnitude of the charge of an electron, and therefore the electron’s mass.

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6
Q

Plum pudding model

A

Thompson; electrons sit amongst positively charged matter

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7
Q

Gold Foil experiment

A

Ernest Rutherford, 1909. Fired alpha particles (tiny positively charged particles) at a thin piece of gold. Most particles went through the gold foil to the detector on the opposite side, but 1 in 8000 particles were deflected at some angle with high energy. Concluded that the atom is mainly empty space and that all the positive charge must be concentrated in a tiny dense nucleus at the centre of the atom

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8
Q

Subatomic particles, mass, charge

A

Protons (1.6710^(-24)g, +1.60210^(-19)C); electrons (9.1210^(-28)g, -1.60210^(-19)C); neutrons (1.67*10^(-24)g, no charge)

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9
Q

Atom’s mass number

A

Protons + neutrons; each nucleon = 1 atomic mass unit (amu); neutrons in nucleus can vary

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10
Q

Isotope

A

Atoms of a given element with different numbers of neutrons

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11
Q

Atomic number

A

Number of protons in an atom

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12
Q

Electric charge of an atom

A

Number of protons - number of electrons

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13
Q

Nuclide symbol

A

Chemical symbol for the element in the centre, atomic number in the subscript to the left, mass number in superscript to the left, charge in superscript to the right

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14
Q

Isotopes of hydrogen

A

Hydrogen-1 (0 neutrons) called protium, Hydrogen-2 (1 neutron) called deuterium, Hydrogen-3 (2 neutrons) called tritium. Not found in equal abundance, have different stabilities. Most hydrogen is hydrogen-1

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15
Q

Isotopes of carbon

A

Carbon-12 (6 neutrons), Carbon-13 (7 neutrons), Carbon-14 (8 neutrons). Most carbon is carbon-12

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16
Q

Atomic mass

A

Have decimal places. Average mass of an atom of a particular element, taking in to account the relative abundance of all the isotopes of the specific element. Atomic mass is determined by multiplying each mass number of an isotope by its relative abundance, and then add them. Units are amu.

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17
Q

Monoatomic ion

A

Singular atom with a formal charge

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18
Q

Polyatomic ion

A

Molecule with a formal charge

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19
Q

Ionic compound

A

Formed by cations and anions being attracted to each other. Cation + Anion; Monoatomic metal cation + Polyatomic anion

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20
Q

Neutral compound

A

Formed when metals and nonmetals come together in a specific ratio. The amount of positive and negative charge must cancel out

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21
Q

Ammonium ion

A

NH4(+)

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22
Q

Acetate ion

A

C2H3O2(-)

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23
Q

Carbonate ion

A

CO3(2-)

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24
Q

Chlorate ion

A

ClO3(-)

25
Q

Chlorite ion

A

ClO2(-)

26
Q

Chromate ion

A

CrO4(2-)

27
Q

Cyanide ion

A

CN(-)

28
Q

Dichromate ion

A

Cr2O7(2-)

29
Q

Hydrogen carbonate ion

A

HCO3(-)

30
Q

Hydrogen sulfate ion

A

HSO4(-)

31
Q

Hydroxide ion

A

OH(-)

32
Q

Hypochlorite ion

A

ClO(-)

33
Q

Nitrate ion

A

NO3(-)

34
Q

Nitrite ion

A

NO2(-)

35
Q

Perchlorate ion

A

ClO4(-)

36
Q

Permanganate ion

A

MnO4(-)

37
Q

Phosphate ion

A

PO4(3-)

38
Q

Sulfate ion

A

SO4(2-)

39
Q

Sulfite ion

A

SO3(2-)

40
Q

Transition metals

A

Can have more than one common charge or oxidation state. Distinguished with Roman numerals

41
Q

Covalent compounds AKA molecular compounds

A

Nonmetals bound to nonmetals. Several numerical combinations possible. Consists of binary molecular compounds, binary acids and oxyacids

42
Q

Binary molecular compound

A

When 2 elements form a molecular compound; A(subscript x)B(subscript y)

43
Q

Prefixes for molecular compounds

A

Mono, di, tri, tetra, penta, hexa, hepta, octa

44
Q

Binary acids and naming

A

HA; contains hydrogen and one other element. Going from the gas to aqueous form, make the following changes to the acid name: change hydrogen to hydro, the second nonmetal has the suffix “-c” and the word “acid” is added to the end. Ex. Hydrogen fluoride gas dissolved in water becomes hydrofluoric acid (aqueous)

45
Q

Oxyacids

A

HOA; contains hydrogen, oxygen and at least one other element. Its molecular structure must allow for acidity. Usually hydrogen atom(s) + oxygen-containing polyatomic anion. (Ex. In HNO3, the nitrate ion NO3(-) is stable so the conjugate acid of HNO3 is acidic).

46
Q

Naming Oxyacids - suffixes

A

The suffix of the anion changes from “-ate” to “-ic” and add the word “acid” at the end (Ex. Nitric acid).

OR, the suffix of the anion changes from “-ite” to “ous” and add the word “acid” at the end. (Ex. nitrous acid).

47
Q

Hypochlorous acid

A

HClO

48
Q

Chlorous acid

A

HClO2

49
Q

Chloric acid

A

HClO3

50
Q

Perchloric acid

A

HClO4

51
Q

Phosphoric acid

A

H3PO4

52
Q

Bromic acid

A

HBrO3

53
Q

Nitrous acid

A

HNO2

54
Q

Nitric acid

A

HNO3

55
Q

Sulfuric acid

A

H2SO4

56
Q

Sulfurous acid

A

H2SO3

57
Q

Carbonic acid

A

H2CO3

58
Q

Acetic acid

A

CH3COOH

59
Q

Number of electrons in energy level

A

2n^2, n = energy level number

DATCrusher Chem Videos (17 decks)

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