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Chemistry 1 PAP > 1st Six Weeks > Flashcards

1st Six Weeks Flashcards

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1
Q

Antimony

A

Symbol: Sb
Atomic Number: 51
Molar Mass: 121.75
Electron Configuration: [Kr] 5s^2 4d^10 5p^3

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2
Q

Arsenic

A

Symbol: As
Atomic Number: 33
Molar Mass: 74.92
Electron Configuration: [Ar] 4s2 3d10 4p3

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3
Q

Barium

A

Symbol: Ba
Atomic Number: 56
Molar Mass: 137.33
Electron Configuration: [Xe] 6s^2

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4
Q

Bismuth

A

Symbol: Bi
Atomic Number: 83
Molar Mass: 208.98
Electron Configuration: [Xe] 6s^2 5d^10 4f^14 6p^3

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5
Q

Bromine

A

Symbol: Br
Atomic Number: 35
Molar Mass: 79.90
Electron Configuration:

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6
Q

Calcium

A

Symbol: Ca
Atomic Number: 20
Molar Mass: 40.08
Electron Configuration:

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7
Q

Carbon

A

Symbol: C
Atomic Number: 6
Molar Mass: 12.01
Electron Configuration:

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8
Q

Chlorine

A

Symbol: Cl
Atomic Number:
Molar Mass:
Electron Configuration:

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9
Q

Chromium

A

Symbol: Cr
Atomic Number: 24
Molar Mass: 52.00
Electron Configuration:

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10
Q

Cobalt

A

Symbol: Co
Atomic Number: 27
Molar Mass: 58.93
Electron Configuration:

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11
Q

Copper

A

Symbol: Cu
Atomic Number: 29
Molar Mass: 63.55
Electron Configuration:

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12
Q

Fluorine

A

Symbol: F
Atomic Number: 9
Molar Mass: 19.00
Electron Configuration:

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13
Q

Gold

A

Symbol: Au
Atomic Number: 79
Molar Mass: 196.97
Electron Configuration:

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14
Q

Iodine

A

Symbol: I
Atomic Number: 53
Molar Mass: 126.91
Electron Configuration:

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15
Q

Iron

A

Symbol: Fe
Atomic Number: 26
Molar Mass: 55.85
Electron Configuration:

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16
Q

Lead

A

Symbol: Pb
Atomic Number: 82
Molar Mass: 207.2
Electron Configuration:

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17
Q

Magnesium

A

Symbol: Mg
Atomic Number: 12
Molar Mass: 24.30
Electron Configuration:

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18
Q

Manganese

A

Symbol: Mn
Atomic Number: 25
Molar Mass: 54.94
Electron Configuration:

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19
Q

Mercury

A

Symbol: Hg
Atomic Number: 80
Molar Mass: 200.59
Electron Configuration:

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20
Q

Nickel

A

Symbol: Ni
Atomic Number: 28
Molar Mass: 58.69
Electron Configuration:

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21
Q

Nitrogen

A

Symbol: N
Atomic Number: 7
Molar Mass: 14.01
Electron Configuration:

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22
Q

Oxygen

A

Symbol: O
Atomic Number: 8
Molar Mass: 16.00
Electron Configuration:

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23
Q

Phosphorus

A

Symbol: P
Atomic Number: 15
Molar Mass: 30.97
Electron Configuration:

24
Q

Platinum

A

Symbol: Pt
Atomic Number: 78
Molar Mass: 195.08
Electron Configuration:

25
Q

Potassium

A

Symbol: K
Atomic Number: 19
Molar Mass: 39.10
Electron Configuration:

26
Q

Silicon

A

Symbol: Si
Atomic Number: 14
Molar Mass: 28.09
Electron Configuration:

27
Q

Silver

A

Symbol: Ag
Atomic Number: 47
Molar Mass: 107.87
Electron Configuration:

28
Q

Sodium

A

Symbol: Na
Atomic Number: 11
Molar Mass: 22.99
Electron Configuration:

29
Q

Strontium

A

Symbol: Sr
Atomic Number: 38
Molar Mass: 87.62
Electron Configuration:

30
Q

Sulfur

A

Symbol: S
Atomic Number: 16
Molar Mass: 32.06
Electron Configuration:

31
Q

Tin

A

Symbol: Sn
Atomic Number: 50
Molar Mass: 118.71
Electron Configuration:

32
Q

Titanium

A

Symbol: Ti
Atomic Number: 22
Molar Mass: 47.90
Electron Configuration:

33
Q

Tungsten

A

Symbol: W
Atomic Number: 74
Molar Mass: 183.85
Electron Configuration:

34
Q

Zinc

A

Symbol:
Atomic Number:
Molar Mass:
Electron Configuration:

34
Q

What is plotted on the x and y axis of a graph?

A

X axis: Independent variable

Y axis: Dependent variable

35
Q

What are the 4 types of evidence for chemical change?

A
  • Temperature change
  • Formation of bubbles
  • Color change
  • Formation of a precipitate
36
Q

What is the difference between a homogenous and heterogenous mixture?

A

Homogenous mixture: a mixture which has uniform composition & properties throughout
Heterogenous mixture: any mixture that is not uniform in composition

37
Q

How can mixtures be separated?

A

Mixtures can be separated by the process of evaporation, which is when a liquid is changed into a gas.

38
Q

What is the difference between extensive and intensive properties? Give examples.

A

An extensive property is one that changes when the size of the sample changes. Ex: mass
An intensive property is a physical one of a system that does not depend on the size or amount of material in the system. Ex: temperature

39
Q

What is the difference between physical and chemical properties? Give examples.

A

A physical property is any property that changes when the size of the sample changes. Ex: color, smell, melting point, etc.
A chemical property is any of a material’s properties that becomes evident during a chemical reaction.
Ex: toxicity, flammability, reactivity, etc.

40
Q

What is precision, accuracy, and uncertainty?

A

Precision: how close a measurement is to other values
Accuracy: how close a measurement is to the actual value
Uncertainty: that which you don’t for certain; the last digit (“doubtful digit”) in any quantitative measurement is uncertain

41
Q

True or false: When using significant figures, you never use the lowest number, if there is one.

A

False: You always use the lowest number if there is one.

42
Q

True or false: Zeros sandwiched between non-zero digits are never significant.

A

False: They are always significant.

43
Q

True or false: Zeros that come before all non-significant zero digits are never significant.

A

True

44
Q

What are physical and chemical changes?

A

Physical change: appearance changes but substance does not
Ex: melting, breaking, cutting, etc.
Chemical change: substance change
Ex: produces bubbles, turns cloudy, change in smell or taste, etc.

45
Q

States of matter

A

Solid- molecules are closely packed, has a fixed position, rigid, cannot be squashed, has a fixed shape, cannot flow, and has a fixed volume (ex: computer)
Liquid- molecules are closely packed (not as much as solids), not rigid, cannot be squashed, has no fixed shape, has a fixed volume, & can flow (ex: water)
Gas- molecules are not closely packed (far apart), not rigid, can be squashed, has no fixed shape/volume, fill the whole space they’re in (ex: helium)
(4th state of matter)

46
Q

Base units

A 
Measure any physical quantity (ex: length) 
meter (m) -> length
kilogram (kg) -> mass
second (s) -> time
mole (mol) -> amount of substance
Kelvin (K) -> temperature
cubic meter (m^3) -> volume
47
Q

Measurements

A 
1 mL = 1 cm^3 = 1 cc (volume)
1 L = 1,000 cm^3
1,000 L = 1 m^3
mm = milliliter
cm = centimeter
nano (n) = 10^-9
micro = 10^-6
milli (m) = 10^-3
centi (c) = 10^-2
kilo (k) = 10^3
mega (M) = 10^6
Angstrom = 10^-10
48
Q

Speed

A

Speed = distance/over (meters (m)/seconds (s))

49
Q

What did J.J. Thompson do?

A

He discovered atoms have electrons, which are much smaller

50
Q

What discovered protons and neutrons?

A
  • Protons: Ernest Rutherford (1914)

* Neutrons: James Chadwick (1932)

51
Q

Dalton’s Atomic Theory

A
  1. Elements are composed of minute, discreet, and small particles called atoms.
  2. Atoms of the same elements are different.
  3. Compounds are composed of atoms of more than one element. In any compound, the combo of atoms is in fixed ratio of small whole numbers.
  4. A chemical reaction involves the separation, combination, or rearrangement of atoms. It does not result in the destruction of the atoms, more the certain of other kinds of atoms.
    1) All atoms of a given element are alike but the atoms of one element differ from the atoms of every other element.
    2) All elements are made up of tiny, invisible, indestructible atoms.
    3) Atoms are not created, destroyed, or converted into any other kinds of atoms during chemical reaction. They are simply rearranged into new compounds.
    4) Compounds result from the chemical combination of a specific ratio of atoms or different elements.
52
Q

Law of Multiple Proportions

A

When 2 elements combine in more than one proportion to form 2 or more compounds, the weights of one element that combine with a given weight of the other element are in the ratios of small whole numbers.

53
Q

Electron Discovery

A
  • The Cathode Ray Tube Experiment: J.J. Thompson and coworkers, 1897
  • Dalton’s Atomic Model: “All matter consists of tiny, indivisible particles.
  • Cathode rays must be made up of stuff that is negatively charged.
  • Particles that made up cathode rays are 1,000 times smaller than a hydrogen atom.
  • All different metals give off cathode rays.
  • Atoms have tiny, negatively charged particles inside them = Electrons.
  • Atoms are neutral.
  • There must be a positive charge in the atom to balance out the electrons.
54
Q

Nucleus Discovery

A
  • Hans Geiger, Ernest Marsden, and Ernest Rutherford (1911)
  • alpha particles: tiny, positively charged particles much smaller than an atom.
  • Hard dense nucleus w/positive charge
55
Q

Gold Foil Experiment

A

The Geiger–Marsden experiments (also called the Rutherford gold foil experiment) were a landmark series of experiments by which scientists discovered that every atom contains a nucleus where its positive charge and most of its mass is concentrated.

56
Q

Proton Discovery

A 
1803- John Dalton
•Atoms are made of even smaller particles.
1897- J.J. Thompson
•Positively charged plate- anode
•Negatively charged plate- cathode
•Cathode rays come from cathode
Electron discovered
Ernest Rutherford
•Discovered the atom's nucleus (99% of the atom's weight is concentrated here)
•Discovered the proton
•Atom's nuclear charge = the number of protons in nucleus = atomic number
1932- James Chadwick
•Discovered neutrons
•Helped invent atomic bomb

Chemistry 1 PAP (6 decks)

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