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Physical Science > Exam 3 > Flashcards

Exam 3 Flashcards

Chapters 12-14

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1
Q

True or False: atoms are the building blocks of nature

A

true

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2
Q

how many distinct kinds of atoms have been found to date?

A

118 (90 of which are in nature)

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3
Q

What is an element?

A

any material consisting of only one type of atom

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4
Q

Atoms consist of ____________, ___________, and ____________.

A

protons, neutrons, and electrons

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5
Q

All atoms of the same element have the same number of protons. Which is called the ________ ____________.

A

Atomic Number

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6
Q

The mass of an atom in __________ ______ ________ (amu) is the total number of protons and neutrons in the atom.

A

atomic mass units

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7
Q

What are isotopes?

A

atoms of the same element that have different masses (numbers of neutrons)

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8
Q

What is the periodic table of elements?

A

A highly organized listing of all known elements sorted by groups (columns) and periods (rows).

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9
Q

How is the position of an element determined?

A

The position of an element is determined by its atomic number and what type of element it is: metals, non-metals, and metalloids.

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10
Q

What are the four sections of the periodic table, and what groups do they encompass?

A

Main group: groups 1, 2, 14-18
Transition Metals: Groups 3-13
Inner-transition metals: two rows under the main pt

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11
Q

Where are Alkali metals found?

A

Group 1

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12
Q

Where are Alkaline earth metals found?

A

Group 2

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13
Q

Where are halogens found?

A

Group 7 (technically 17)

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14
Q

Where are noble gasses found?

A

group 8 (technically 18)

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15
Q

Describe metals

A
  • good conductors (bad insulators) of heat and electricity
  • typically shiny
  • malleable and ductile
  • solids at room temperature, with the exception of mercury (liquid at room temp)
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16
Q

Describe nonmetals

A
  • properties are more variable
  • solids, liquids, and gases
  • poor conductors (good insulators) of heat and electricity
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17
Q

describe metalloids

A
  • dull appearing
  • brittle
  • solids
  • sometimes called semiconductors
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18
Q

What is a spectroscope?

A

an instrument that separates and spreads light into its component frequencies

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19
Q

what does a spectroscope allow for?

A

analysis of light emitted by elements when they are made to glow - this identifies each element by its characteristic pattern.

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20
Q

Atomic Excitation: Electron _________ potential and moves farther from the nucleus. A photon of light is _________.

A

gains; absorbed

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21
Q

Atomic Excitation: Electron ________ potential energy and moves closer to the nucleus. A photon of light is _________.

A

loses; emitted

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22
Q

Describe the planetary model of the atom.

A

protons and neutrons are clumped together in the nucleus (the middle of the atom) with electrons orbiting around the nucleus on various levels.

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23
Q

Explain Electron waves

A

An electron’s wave nature explains why electrons in an atom are restricted to particular energy levels.

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24
Q

Describe the shell model of the atom

A

“3-D cutaway view” of an atom (think of how we draw animal cells)

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25
Q

In the electromagnetic force, protons _______ one another.

A

repel

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26
Q

In the nuclear forces, there is an ____________ force between protons and neutrons.

A

attractive

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27
Q

When the strong nuclear force is larger than the electric force, the protons are __________ to one another.

A

attracted

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28
Q

When the strong nuclear force is weaker than the electric force, the protons are ___________ by one another.

A

repelled

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29
Q

The presence of ___________ helps hold the nucleus together.

A

neutrons

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30
Q

What are the three types of nuclear reactions?

A

Radioactivity (a small piece of the nucleus leaves the atom)
Fission (“splitting the atom”)
Fusion (two small atoms combine into one larger atom)

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31
Q

What is Transmutation?

A

the conversion of one element to another element through the process of radioactive decay.

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32
Q

What is a half-life?

A

The interval of time required for one-half of the atomic nuclei of a radioactive sample to decay.

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33
Q

Iodine-131 has a half-life of 8 days. If you start with 1000g of iodine-131, how much will be left after 32 days?

A

8 days = 500g
16 days = 250g
24 days = 125g
32 days = 62.5g

34
Q

What is radiometric dating?

A

ways of determining the age of objects or materials.

35
Q

How many different radiometric dating methods are there?

A

Over 40; they all give good agreement

36
Q

What is carbon dating used for?

A

plants and animals

based upon ratio of carbon-12 to carbon-14

37
Q

What are nonliving things dated through?

A

uranium and lead isotopes

38
Q

Explain ionizing radiation

A

knocks electrons out of atoms.

39
Q

Explain Free Radicals.

A

An atom or group of atoms with one unpaired electron.

40
Q

Explain stomatic damage

A

the organism exposed to the radiation is affected.

41
Q

explain genetic damage

A

damage to reproductive system affects offspring

42
Q

Most radiation we encounter is:

A

Natural background radiation that originates in Earth and space

43
Q

What is a chain reaction?

A

A chain reaction is a self-sustaining reaction in which the products of one reaction event stimulate further reaction events.

44
Q

Define Critical mass

A

the minimum mass of fissionable material in a reactor or nuclear bomb that will sustain a chain reaction.

45
Q

At or above critical mass, in a large quantity of atoms, an enormous __________ can occur.

A

explosion

46
Q

What is the Mass-Energy Equivalence?

A

E=mc^2
mass is a very large form of pe.
Mass pe can be converted to ke.

47
Q

Produce ________ = used to produce electricity in nuclear reactors/

A

steam

48
Q

Nuclear reactors: what fuels are/can be used?

A

Uranium-235
Plutonium-239

49
Q

What does a control rod do?

A

absorbs extra neutrons to slow down acceleration.

50
Q

In nuclear reactors, nuclear explosion cannot occur because fuel pellets are below critical mass. In a nuclear bomb, two __________ masses are driven together to reach critical mass.

A

subcritical

51
Q

Only ______% of natural Uranium is U-235

A

0.7%

52
Q

Define Nuclear Fusion

A

the combination of nuclei of light atoms to form heavier nuclei with the release of much energy

53
Q

________ is the “nuclear sink” for energy production. Any nuclear transformation that moves nuclei towards iron releases _______.

A

iron; energy

54
Q

Describe thermonuclear fusion

A

nuclear fusion is produced by high temperatures.
mass decreases as energy is released.
source of energy in the starts (sun).

55
Q

What is a problem of fusion power plants?

A

They have really high temperatures (laser?).

Only experimental at this time.

56
Q

What are the two advantages of Fusion Power Plants?

A

Hydrogen (from water) is the fuel source and there is low levels of radioactivity.

57
Q

Define a physical property:

A

A physical property describes the look or feel of a substance.

58
Q

Define a chemical property:

A

A chemical property describes the tendency of a substance to transform into a new substance.

59
Q

What are the 5 signs of a chemical reaction?

A

Change in color
Precipitation
Bubbling (not boiling)
Change in temp.
Evolution of light

60
Q

What is an element?

A

A material made of only one kind of atom.

61
Q

What is the elemental formula?

A

The elemental formula is used to show the proportion by which atoms combine to form an element.

62
Q

What is a compound?

A

A substance consisting of atoms of different elements.

63
Q

____________ have properties uniquely different from the elements from which they are made.

A

Compounds

64
Q

What is a chemical formula?

A

A chemical formula is used to show the proportion by which elements combine to form a compound.

65
Q

Are these elements or compounds?
1. Cl2
2. H2O
3. CCl4
4. C60
5. PBr3

A
  1. element
  2. compound
  3. compound
  4. element
  5. compound
66
Q

What is the first guideline to naming compounds?

A

Used when elements are on opposite sides of the periodic table (a metal and a nonmetal). Start with the element farthest to the left in the periodic table, then, for the element to the right, add the suffix -ide.

67
Q

Name this compound: NaCl

A

Sodium Chloride

68
Q

Name this compound: KF

A

Potassium flouride

69
Q

Name this compound: CaBr2

A

Calcium Dibromide

70
Q

Name this compound: BaO

A

Barium oxide

71
Q

Name this compound: Cs2S

A

Dicesium sulfide

72
Q

What is the second guideline to naming compounds?

A

Used when both elements are on the same side of the periodic table (usually both are nonmetals). With different possible combinations of elements, use prefixes to remove ambiguity.

73
Q

What are the five prefixes used for guideline 2?

A

1 = mono
2 = di
3 = tri
4 = tetra
5 = penta

74
Q

Name this compound: CO

A

Carbon monoxide

75
Q

Name this compound: CO2

A

Carbon dioxide

76
Q

Name this compound: CCl4

A

Carbon tetrachloride

77
Q

Name this compound: NO2

A

Nitrogen dioxide

78
Q

Name this compound: PBr3

A

Phosphorus tribromide

79
Q

Name this compound: N2O4

A

Dinitrogen tetroxide

80
Q

What is the third guideline for naming compounds?

A

Name is not systematic. It is a “common name”.

81
Q

Name this compound: H2O

A

“Water”
dihydrogen monoxide

82
Q

Name this compound: H2O2

A

“Hydrogen Peroxide”
dihydrogen dioxide

Physical Science (5 decks)

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