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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
What did Geiger and Marsden do?
Tested the plum pudding model - discovered + charged nucleus where most of the mass of the atom is held
26
The positively charged center of an atom that contains nearly all the atoms mass
Nucleus
27
A positively charged subatomic particle present in the nucleus of an atom
Proton
28
An electronically neutral subatomic particle found in the nucleus of the atom
Neutron
29
Who discovered and characterized free neutrons to make the model of the atom complete?
James Chadwick
30
Unit used to express the relative masses of atoms and subatomic particles
Atomic mass unit (amu)
31
A unit of mass identical to 1 atomic mass unit
Daltons
32
Who published the 1st table of atomic masses?
John dalton
33
Who built modified cathode ray tubes that were evacuated except for small quantities of fill gases?
Francis W Aston
34
An atom or group of atoms that has a net positive or negative charge
Ion
35
Atoms of an element containing different numbers of neutrons
Isotopes
36
The nucleus of a specific isotope of an element
Nuclide
37
The # of protons in a nucleus of an atom
Atomic # (Z)
38
Either a proton or a neutron in a nucleus
Nucleon
39
The number of nucleons (proton plus neutron) in an atom
Mass number
40
Chart of the elements in order of their atomic #s and in a pattern based on their physical and chemical properties
Periodic table of elements
41
Who- Theory of chemical atomism- matter is composed of atoms and atoms are indivisible and indestructible
John Dalton
42
Discovered radioactivity and isolated the previously unknown elements polonium and radium
Marie curie
43
Proved that atoms are made up of smaller particles
Marie curie
44
Spontaneous emission of energy and particles from atomic nuclei
Radioactivity
45
For neutral atoms, the number of what equals the number of what
Protons = electrons
46
Defined as exactly 1/2 the mass of a carbon-12 atom
1 amu
47
"Electrons are distributed through a uniformly charged (+) sphere of atomic dimensions
JJ Thomson
48
Describe the plum pudding model
Electrons are like raisins dispersed in a (+) charged pudding could
49
Who determined the charge to mass ratio of an electron
JJ Thomson
50
Who performed experiments involving charged oil drops and determined the mass of the electron?
Robert Andrews Milikan
51
Who tested Thomsons pp model? How?
Rutherford | Directed alpha particles at metal foil pieces and found that some deflected back at high angles- discovered nucleus
52
Who created the "nuclear model"
Rutherford
53
Atom is a dense center of positive charge surrounded by electrons
Nuclear model
54
All atoms of an element have the same number of what?
Protons
55
The # of protons in the nucleus
Atomic #
56
Tells us the mass of one atom of an element RELATIVE to one atom of another element
Atomic weight
57
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
Average atomic mass
58
The proportion of a particular isotope, usually expressed as a percent, relative to all the isotopes of that element In a natural sample
Natural abundance
59
Equation for average atomic mass
Mass of each isotope x natural abundance and then sum the weighted masses
60
Who showed that subjecting a mixture of gasses present in earths early atmosphere to an electric current could produce amino acids
Harold Urey and Stanley Miller
61
A substance consumed during a chemical reaction
Reactant
62
A substance formed during a chemical reaction
Product
63
What do chemical equations describe?
Reactions
64
A reaction in which two (or more) substances combine to form one product
Combination reaction
65
An amount of material that contains Avogadro's number of particles
Mole
66
The # of carbon atoms in exactly 12 grams of the carbon 12 isotope
Avogadro's number
67
The mass of 1 mole of a substance
Molar mass
68
Sum of protons + neutrons for an atom
Mass number
69
Atoms of the same element but different mass number
Isotopes
70
Number of atoms of a given isotope divided by total number of all atoms of all isotopes of the element x 100
Percent abundance
71
Experimentally determined mass of an atom of one isotope
Exact mass of isotope
72
Determination of masses of isotopes | Weighted average of atoms in a natural sample of element
Mass spectrometer
73
One mole always contains the same (blank), no matter the substance
Number of particles
74
Avogadro's number
6.022 x 10^23 particles
75
Mass in grams of one mole of a substance
Molar mass
76
Who created the first periodic table?
Dmitri Mendeleev
77
How did Mendeleev arrange elements?
Based on similar chemical properties and increasing atomic mass

Chemisty (10 decks)

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