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Gen Chem > Gen Chem 1-2 > Flashcards

Gen Chem 1-2 Flashcards

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1
Q

First coined the term “atomos” or “uncuttable”

A

Democritus

Mnemonics: Democritus : Atomos

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2
Q

Hypothesized atomic theory

-

A

John Dalton

Mnemonics: Dalton’s Atomic Theories (4 DAT)

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3
Q

4 Dalton’s Hypotheses on Atomic Theory?

A
  1. Elements (w/atoms)
  2. Unique atoms per element
  3. Compounds (w/ > 1 element)
  4. Law of Conservation of mass

Mnemonics: EUCL (Dalton’s 4 Ukelele)

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4
Q

“When** two elements **combine to form more than one compound, weights of the elements are in ratio of small integers”

What do you call this law?
Who is the proponent? **

C + O = CO2

C + O = CO

A

Law of Multiple Proportions
(John Dalton)

Mnemonics: Lumps (LMP) ni Dalton

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5
Q

“Same chemical compound,
always same mass proportion of elements”

What do you call this law?
Who is the proponent?

Any sample of water contains 11.19% H and 88.81% O, by mass.

A

Law of Definite Proportions
(Joseph Louise Proust)

Mnemonics: (LDP) DEFINITE mag Pro-PROUST

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6
Q

First isolated sugar from grapes

A

Joseph Louis Proust

Mnemonics: Proust as a Sugar Daddy

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7
Q

“When body energy changes by an amount E , the mass (m) of the body will change by an amount equal to E/c2.”

Who is the proponent of this theory?

Mass-energy - Energy Lost : Mass Lost

A

Albert Einstein

Mnemonics :Mass-energy - Energy Lost : Mass Lost

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8
Q

Emission- Transmission of energy in space

Form: Wave

A

Radiation

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9
Q

It is a vacuum tube containing one or more electron guns – emit electron beams that are manipulated to display images on a phosphorescent screen.

Invisible ray –> coated surface –> FLUORESCENCE

A

Cathode Ray Tube

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10
Q

In a CRT:

Anode:
Cathode:

Plate Charges

A

In a CRT:
Anode: (+) positively charged plates
Cathode: (-) negatively charged plates

Mnemonics: A+ C-

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11
Q

What is the “eletric charge to mass” ratio?

JJ Thomson

A

( - 1.76 x 10^8 C/g)

Mnemonics: 678 pero shuffled
Positive value exponent

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12
Q

What is the value for electron (e -) charge?

A

( - 1.6022 x 10 ^ -19)

Mnemonics: -16, -19, 022

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13
Q

1923 Nobel Prize in Physics - determining electron (e -) charge

American P

A

Robert Millikan

Mnemonics: May Electron Charge ang Gatas ni Robert

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14
Q

1906 Nobel Prize Physics for discovery of electron

British P

A

JJ Thomson

RE: Plum-Pudding Model (Positive sphere, Negative Raisins)

Mnemonics: Nega si JJ

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15
Q

Given Real Constants:

(A) electron charge = - 1.6022 x 10^-19 C
(B) ratio e charge/mass = -1.76 x 10^8 C/g

Find the mass of electron.

mass electron = A/B

A

9.10x^-28 g

Mnemonics: Mass e - : 9, 10, 28 (negative exponent)

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16
Q

1901 Nobel Prize Physics - discovery of X-Rays (a.k.a. Rontgen Rays)

X-Rays
- darkened photographic plates
- can’t be deflected by

German P

A

Wilhelm Konrad Rontgen

Mnemonics: X-Rays (a.k.a. Rontgen Rays)

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17
Q

3 Types of raays emitted by decay of radioactives?

e.g. Uranium

A

α rays (+)
β rays (-)
γ rays (no charge)

X-Ray : gamma ray

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18
Q

1903 Nobel Prize Physics (1/2) - discovery of uranium radioactivity

French P

A

Antoine Henri Becquerel

Mnemonics: Bekenemen Uranium

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19
Q

Spontaneous emission of particles

Coined by Marie Curie

A

Radioactivity

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20
Q

1903 Nobel Prize Physics (1/2) - Radioactivity
1911 Nobel Prize Chemistry - Radium & Polonium

A

Marya Sklodowska

Marie Curie

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21
Q

1908 Nobel Prize Chemistry - investigation & discovery of atomic nucleus

Nucleus: proton-dense central core in atom

Mnemonic: R with GuM

New Zealand, German, & English P

A

Ernest Rutherford
with:
associate Johannes Geiger
undergrad Ernest Marsden

Different languages, PAANO SILA NAG COMMUNICATE TE?

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22
Q

Measures RADIATION

A

Geiger Counter

Mnemonics: Counter Radiation ni Geiger

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23
Q

Invented Geiger Counter

German P

A

Johannes Hans Wilhem Geiger

Mnemonics: JHWG or simply MONSTER Anime (Brain Surgery)

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24
Q

Charge of a Proton is equal to ___________

Value? Comparison?

A

+1.6022x10^-19 C

Same with electron (tho, different signs)

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25
Q

Unit for Electric Charge

A

Coulomb

Mnemonics: CC (Coulomb - Charge)

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26
Q

Nucleus covers ____ volume of an atom

Mnemonics: Stadium: Atom & Small Marble: Nucleus

A

(1/10)^13

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27
Q

Unit of atomic dimension

Mnemonics: Dimensions ba kamo? PM Sent

A

Picometer (pm)

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28
Q

1 picometer (pm) is equal to ____ m

Mnemonics: Negative dozen

A

1 x 10^-12

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29
Q

1 angstrom (Å) is equal to ____ picometer (pm)

ANGSTROM is a non-SI unit for atomic length

A

100 picometer

Mnemonics: 1 AM - 100 PM

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30
Q

Radius of atomic nucleus

Value in picometers?

A

5 x 10 ^ -3 pm

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31
Q

What is the missing part of Rutherford’s Model?

A

Neutrons

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32
Q

1935 Nobel Prize Physics - discovery of neutron (slightly denser >proton)

A
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33
Q

What is the ratio of Helium to Hydrogen atoms?

A

4:1

Helium has 2P, 2N while Hydrogen has 1P, 0N

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34
Q

Mass of Subatomic Particles:

m Electron: X
m Proton: Y
m Neutron: Z

Find X , Y , & Z.

P > N > E

A

Mass of Subatomic Particles:

m Electron: 9.109 x 10^ -28
m Proton: 1.673 x 10 ^ -24
m Neutron: 1.675 x 10 ^ -24

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35
Q

Charge of Subatomic Particles:

m Electron: X
m Proton: Y
m Neutron: Z

Find X , Y , & Z.

P > E > N

A

Charge of Subatomic Particles:

m Electron: - 1.6022 x 10 ^ -19
m Proton: + 1.6022 x 10 ^ -19
m Neutron: 0

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36
Q

Number of protons in nucleus the ___?

Mnemonics: P = E = Z

A

Atomic Number (Z)

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37
Q

Is number of proton equal to electrons?

A

Yes

P = E

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38
Q

Total number of protons and neutrons in nucleus is ____?

Mnemonics 1: P + N = A

A

Mass Number (A)

Mnemonics 2: P + N = A

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39
Q

How to get neutron number?

A

N = A - Z

Mnemonics: Nazi

40
Q

Boron:
Mass Number = 12
P: ?
E: ?
N: ?

A

Boron:
Mass Number (A) = 12
(Z) P: 5
(Z) E: 5
N: 7

N = A - Z

41
Q

What do you call atoms with same atomic number, but different mass numbers?

Same Z, Different A

A

Isotopes

42
Q

3 Isotopes of Hydrogen

A

Protium (H-1): 1P, 0N
Deuterim (H-2): 1P, 1N
Tritium (H-3): 1P, 2N

43
Q

2 Common Isotopes of Uranium

A

Uranium- 235
Uranium - 238

Both Z = 92

Atomic # Uranium : 92

44
Q

Isotopes of Elements are determined by their ____ numbers?

A

Mass Numbers

Isotopes = A

45
Q

Na
Mass Number (A): 20
Atomic Number (Z): 11
P: ?
E: ?
N: ?

A

Na
Mass Number (A): 20
Atomic Number (Z): 11
P: 11
E: 11
N: 9

46
Q

O
Mass Number (A): 17
P: ?
E: ?
N: ?

A

O
Mass Number (A): 17
Atomic Number (Z): 8
P: 8
E: 8
N: 9

47
Q

Carbon-14
P: ?
E: ?
N: ?

A

Carbon-14
Mass Number (A): 14
Atomic Number (Z): 6
P: 6
E: 6
N: 8

48
Q

Cu
Mass Number (A): 63
P: ?
E: ?
N: ?

A

Cu
Mass Number (A): 63
Atomic Number (Z): 29
P: 29
E: 29
N: 34

49
Q

Name the only element with an isotope of zero nucleus

A

Hydrogen

50
Q

Why helium nucleus with zero neutron is likely to be unstable?

Forces

A

The remaining protons will repel electromagnetically, causing atom to fall apart.

51
Q

Horizontal: Periods
Vertical : ___________

Periodic Table

A

Groups/ Families

52
Q

3 Categories of Elements

A

Metal, Nonmetal, Metalloid

53
Q

Group 1A Elements : _____

A

Alkali Metals

(Li, Na, K, Rb, Cs, Fr)

Mnemonics: ULi Na Ka, Robinsons’ Ces, For Real?

54
Q

Group 2A elements: __________

A

Alkaline Earth Metals

(Be, Mg, Ca, Sr, Ba, Ra)

Mnemonics: Be Mag Canton mi ni Sir IBaRa

55
Q

In the periodic table, do chemical properties changes more markedly across a period or down a group?

A

Across a period

56
Q

It is an aggregate of a least 2 atom in a definite arrangement (held together by chemical bonds)

Hydrogen gas (H-H) , these are neural substances

A

Molecule

LDP: may contain atoms of same element or diff. yet in small ratio

57
Q

Diatomic molecules can be compose of atoms of 2 different elements. True or False?

A

True

HCl, CO, H2, N2, Cl2, Br2,

58
Q

Molecules containing more than 2 atoms

A

Polyatomic molecules

59
Q

Ozone (O3), H2O, Ammonia (NH3) are what type of molecules?

A

Polyatomic molecules

60
Q

Which of the following does not exist as a diatomic molecule?

H, N, O, F, Cl, Br, I

A

None of the above

61
Q

Atoms with net positive/negative charge?

A

Ions

62
Q

Number of protons changes during chemical reactions. True or False?

A

False. It remains the same.

63
Q

Metal: Cation: Loses electrons
Nonmetal: Anions: _______- electrons

A

Gains

64
Q

Compounds formed from cations and anions?

A

Ionic Compounds

65
Q

Used by chemist to express composition of molecules and ionic compounds in terms of chemical symbol

A

Chemical Formulas

66
Q

2 Types of Chemical Formulas?

A

Molecular Formulas
Empirical Formulas

67
Q

Type of chemical formula that shows exact # of atoms of each element

A

Molecular Formula

Mnemonics: Molecu(LAHART)???

68
Q

1 of 2 or more distinct forms of an element

A

Allotropes

69
Q

2 Allotropes of Carbon

A

Diamond
Graphite

Mnemonics: Carbon-DG

70
Q

Difference between ball-and-stick and space-filling molecular models?

A

The latter is more accurate; shows variation of atomic size

71
Q

Type of chemical formula that shoes which elements are present in simplest ratio of atoms.

A
72
Q

HydraziNe
Molecular Formula: ?
Empirical Formula: ?

Clue: H N (EVEN REVERSED)

A

HydraziNe
Molecular Formula: N2H4
Empirical Formula: NH2

73
Q

CHLoroform
Molecular Formula: ?
Empirical Formula: ?

Clue: C, H, CL (3)

A

CHLoroform
Molecular Formula: CHCl3
Empirical Formula: CHCl3

74
Q

AceTYlene
Molecular Formula: ?
Empirical Formula: ?

Clue: C, H (ACE-TWO-LENE)

A

AceTYlene
Molecular Formula: C2H2
Empirical Formula: CH

75
Q

Glucose
Molecular Formula: ?
Empirical Formula: ?

Clue: C, H, O (121)

A

Glucose
Molecular Formula: C6H12O6
Empirical Formula: CH2O

76
Q

CAFFEINE
Molecular Formula: ?
Empirical Formula: ?

Clue: CHNO (not chons) 8, 10, 4, 2

A

Caffeine
Molecular Formula: C8H10N4O2
Empirical Formula: C4H5N2O

77
Q

Guess the Ionic Compound Formula:
Potassium Bromide
Zinc Iodide
Aluminum Oxide

A

KBr
ZnI2
Al2O3

K+, Br-, Zn2+, I-, Al3+, O2-

78
Q

Guess the Ionic Compound Formula:
Magnesium Nitride
Chromium Sulfate
Titanium Oxide

Titanium (4 ; syllables daw = charge)

A

Mg3N2
Cr2(SO4)3
TiO2 (Simplied by factor of 2)

Mg2+, N3-, Cr3+, (SO4)2-, Ti4+, O2-

79
Q

Inorganic compounds contains C,H,O,N,S? True or False

A

False. Organic

80
Q

5 Divisions of naming Inorganic Compounds

Mnemonics: I’M A BitcH

A

Ionic Compounds
Molecular Compounds
Acids
Bases
Hydrates

Mnemonics: I’M A BitcH

81
Q

Name compounds that is an exception in naming ionic compounds

Not a metal nor nonmetal

A

Ammonium Ion
(NH4+)

82
Q

2 Step in Naming Ionic Compounds

A

S1. Name the metal
S2. change nonmetal to -ide

83
Q

Can transition metal form more than 1 type of cation? True or False?

A

True

84
Q

Ionic Compound Naming
FeCl2 : ________
FeCl3:________

A

Ionic Compound Naming
FeCl2 : ferrOUS chloride
FeCl3: ferrIC chloride

85
Q

Ionic Compound Naming
Cu2+: ________

A

Ionic Compound Naming
Cu2+: cuprIC

86
Q

Ionic Compound Naming via STOCK
Mn2+: ________
Mn3+: ________
Mn4+: ________

MANGA 2,3,4,

A

Mn2+: MnO
Mn3+: Mn2O3
Mn4+:MnO2

manganese (XX) oxide

87
Q

Name the following:
Cu(NO3)2
KH2PO4
NH4ClO3

Ionic

A

Copper (II) nitrate
Potassium dihydrogen phosphate
Ammonium chlorate

88
Q

State the chemical formulas:
mercury (I) nitrate
cesium sulfide
calcium phosphate

rubidium sulfate
barium hydride

A

Hg2(NO2)2
Cs2S
Ca3(PO4)2

Rb2SO4
BaH2

Hg2+, NO2-, Cs+, S2-, Ca2+, (PO4)3-, Rb2+, (SO4)2-, Ba2+, H-

89
Q

Which type of inorganic compounds uses greek prefixes in naming the molecular compounds

Particularly, second element?

A

Molecular (Covalent) Compounds

Nonmetal-Nonmetal

Drop mono, Drop “a” in prefix

90
Q

Name these 3 common covalent compounds:
B2H6: ?
SiH4: ?
PH3: ?

A

B2H6: DIBORANE (2 BORINGGG)
SiH4: SILANE (SILICON IN 4 LANES)
PH3: **PHOSPHINE ** (PUSPIN :3)

91
Q
A
92
Q
A
93
Q
A
94
Q
A
95
Q
A

Gen Chem (2 decks)

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