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Chemisty > Unit 2 Notes > Flashcards

Unit 2 Notes Flashcards

1
Q

Why do we use atomic mass units (amu)?

A

It is used to express the relative masses of atoms and subatomic particles. It would be really hard to measure a single atom in grams.

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2
Q

What are isotopes?

A

Atoms of an element containing different numbers of neutrons?

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3
Q

Do the number of protons change with different isotopes?

A

No

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4
Q

What is Avogadro’s number?

A

6.022 x 10^23 particles/mole

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5
Q

What is molar mass?

A

Mass in grams of one mole of a substance

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6
Q

The (blank) determines on element from another. In other words the # of (blank) determines one element from another.

A

Atomic #

Protons

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7
Q

In determining molecular mass, we multiply the experimentally determined masses of each isotope by their

A

% natural abundance

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8
Q

How do isotopes differ?

A

of neutrons

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9
Q

What are the 3 different isotopes of hydrogen?

A

Hydrogen/protium h,1,1
Deuterium h,2,1
Tritium h,3,1

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10
Q

How do you calculate the average atomic mass of an element?

A

Atomic mass x percent abundance + atomic mass x percent abundance

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11
Q

Kinetic molecular theory relates to what?

A

The drawing of solids, liquids, and gasses and the particles

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12
Q

All matter consists of (blank)

A

Atoms

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13
Q

Who discovered electrons using a cathode-Ray tube

A

JJ Thomson

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14
Q

Who was not sure where electrons fit into the structure of atoms?

A

JJ Thomson

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15
Q

Streams of electrons emitted by the cathode in a partially evacuated tube

A

Cathode rays

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16
Q

Subatomic particle that has a negative charge and essentially zero mass

A

Electrons

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17
Q

Who calculated the mass of the electron?

A

Robert Milikan

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18
Q

Who created the plum pudding model?

A

JJ Thomson

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19
Q

Who discovered radiation from Uranium?

A

Henri Becquerel

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20
Q

Who showed radiation containing particles and rays?

A

Curie and Rutherford

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21
Q

Spontaneous emissions of high energy radiation and particles by materials

A

Radioactivity

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22
Q

Who calculated the mass to charge ratios?

A

Rutherford

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23
Q

A radioactive emission that is a high energy electron

A

Beta particle

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24
Q

A radioactive emission with a charge of Z+ and a mass equivalent to that of a helium nucleus

A

Alpha particle

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25
Q

What did Geiger and Marsden do?

A

Tested the plum pudding model - discovered + charged nucleus where most of the mass of the atom is held

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26
Q

The positively charged center of an atom that contains nearly all the atoms mass

A

Nucleus

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27
Q

A positively charged subatomic particle present in the nucleus of an atom

A

Proton

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28
Q

An electronically neutral subatomic particle found in the nucleus of the atom

A

Neutron

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29
Q

Who discovered and characterized free neutrons to make the model of the atom complete?

A

James Chadwick

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30
Q

Unit used to express the relative masses of atoms and subatomic particles

A

Atomic mass unit (amu)

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31
Q

A unit of mass identical to 1 atomic mass unit

A

Daltons

32
Q

Who published the 1st table of atomic masses?

A

John dalton

33
Q

Who built modified cathode ray tubes that were evacuated except for small quantities of fill gases?

A

Francis W Aston

34
Q

An atom or group of atoms that has a net positive or negative charge

A

Ion

35
Q

Atoms of an element containing different numbers of neutrons

A

Isotopes

36
Q

The nucleus of a specific isotope of an element

A

Nuclide

37
Q

The # of protons in a nucleus of an atom

A

Atomic # (Z)

38
Q

Either a proton or a neutron in a nucleus

A

Nucleon

39
Q

The number of nucleons (proton plus neutron) in an atom

A

Mass number

40
Q

Chart of the elements in order of their atomic #s and in a pattern based on their physical and chemical properties

A

Periodic table of elements

41
Q

Who- Theory of chemical atomism- matter is composed of atoms and atoms are indivisible and indestructible

A

John Dalton

42
Q

Discovered radioactivity and isolated the previously unknown elements polonium and radium

A

Marie curie

43
Q

Proved that atoms are made up of smaller particles

A

Marie curie

44
Q

Spontaneous emission of energy and particles from atomic nuclei

A

Radioactivity

45
Q

For neutral atoms, the number of what equals the number of what

A

Protons = electrons

46
Q

Defined as exactly 1/2 the mass of a carbon-12 atom

A

1 amu

47
Q

“Electrons are distributed through a uniformly charged (+) sphere of atomic dimensions

A

JJ Thomson

48
Q

Describe the plum pudding model

A

Electrons are like raisins dispersed in a (+) charged pudding could

49
Q

Who determined the charge to mass ratio of an electron

A

JJ Thomson

50
Q

Who performed experiments involving charged oil drops and determined the mass of the electron?

A

Robert Andrews Milikan

51
Q

Who tested Thomsons pp model? How?

A

Rutherford

Directed alpha particles at metal foil pieces and found that some deflected back at high angles- discovered nucleus

52
Q

Who created the “nuclear model”

A

Rutherford

53
Q

Atom is a dense center of positive charge surrounded by electrons

A

Nuclear model

54
Q

All atoms of an element have the same number of what?

A

Protons

55
Q

The # of protons in the nucleus

A

Atomic #

56
Q

Tells us the mass of one atom of an element RELATIVE to one atom of another element

A

Atomic weight

57
Q

A weighted average of masses of all isotopes of an element, calculated by multiplying the natural abundance of each isotope by its mass in atomic mass units and then summing the products

A

Average atomic mass

58
Q

The proportion of a particular isotope, usually expressed as a percent, relative to all the isotopes of that element In a natural sample

A

Natural abundance

59
Q

Equation for average atomic mass

A

Mass of each isotope x natural abundance and then sum the weighted masses

60
Q

Who showed that subjecting a mixture of gasses present in earths early atmosphere to an electric current could produce amino acids

A

Harold Urey and Stanley Miller

61
Q

A substance consumed during a chemical reaction

A

Reactant

62
Q

A substance formed during a chemical reaction

A

Product

63
Q

What do chemical equations describe?

A

Reactions

64
Q

A reaction in which two (or more) substances combine to form one product

A

Combination reaction

65
Q

An amount of material that contains Avogadro’s number of particles

A

Mole

66
Q

The # of carbon atoms in exactly 12 grams of the carbon 12 isotope

A

Avogadro’s number

67
Q

The mass of 1 mole of a substance

A

Molar mass

68
Q

Sum of protons + neutrons for an atom

A

Mass number

69
Q

Atoms of the same element but different mass number

A

Isotopes

70
Q

Number of atoms of a given isotope divided by total number of all atoms of all isotopes of the element x 100

A

Percent abundance

71
Q

Experimentally determined mass of an atom of one isotope

A

Exact mass of isotope

72
Q

Determination of masses of isotopes

Weighted average of atoms in a natural sample of element

A

Mass spectrometer

73
Q

One mole always contains the same (blank), no matter the substance

A

Number of particles

74
Q

Avogadro’s number

A

6.022 x 10^23 particles

75
Q

Mass in grams of one mole of a substance

A

Molar mass

76
Q

Who created the first periodic table?

A

Dmitri Mendeleev

77
Q

How did Mendeleev arrange elements?

A

Based on similar chemical properties and increasing atomic mass

Chemisty (10 decks)

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