Ch 3 Section 3 Flashcards

1
Q

Atoms are much too small to be

A

Measured individually

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2
Q

Chemists can analyze atoms

A

Quantitatively by knowing fundamental properties of the atoms of each element

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3
Q

Mole

A

A special unit used by chemists to express amounts of particles, such as atoms and molecules

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4
Q

All atoms are composed of the

A

Same basic particles

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5
Q

Atoms of different elements have

A

Different numbers of protons

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6
Q

Atoms of the same element all have the same number of

A

Protons

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7
Q

The atomic number (Z) of an element is

A

The number of protons of each atom of that element

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8
Q

All atoms of the element hydrogen have

A

One proton

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9
Q

The atomic number identifies

A

An element

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10
Q

The simplest atoms are those of

A

Hydrogen

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11
Q

Like many naturally occurring elements hydrogen atoms can have

A

Different numbers of neutrons

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12
Q

The most common type of hydrogen is sometimes called

A

Protium

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13
Q

Protium accounts for

A

99.9885% of the hydrogen atoms found on earth

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14
Q

The nucleus of a protium atom consists of

A

One proton only and it had one electron moving about it

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15
Q

Another form of hydrogen is deuterium which accounts for

A

0.0115% of earths hydrogen atoms

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16
Q

Each deuterium atom has a

A

Nucleus with one proton and one neutron

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17
Q

The third form of hydrogen is known as tritium which is

A

Radioactive

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18
Q

Tritium exists in very small

A

Amounts in nature but can be prepared artificially

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19
Q

Each tritium atom has one

A

Proton, two neutrons, and one electron

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20
Q

Isotopes are atoms of the same element that have

A

Different masses

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21
Q

The isotopes of a particular element all have the same number of

A

Protons and electrons but different numbers of neutrons

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22
Q

Most of the elements consist of

A

Mixtures of isotopes

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23
Q

Identifying an isotope requested knowing both the

A

Name or atomic number of the element and the mass of the isotope

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24
Q

The mass number is the

A

Total number of protons and neutrons that make up the nucleus of an isotope

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25
Isotopes are usually identified by
Specifying their mass number
26
There are two methods for
Specifying isotopes
27
In the first method the mass number is written with a
Hyphen after the name of the element (hyphen notation)
28
The second method shows the composition of a
Nucleus using the isotopes nuclear symbol
29
The superscript in nuclear symbol indicates the
Mass number (protons + neutrons)
30
The subscript in nuclear symbol indicates the
Atomic number (number of protons)
31
The number of neutrons is found by
Subtracting the atomic number from the mass number
32
Nuclide is a general term for a
Specific isotope of an element
33
Masses of atoms expressed in grams are
Very small
34
For most chemical calculations it is more convenient to use
Relative atomic masses
35
In order to set up a relative scale of atomic mass one atom has been
Arbitrarily chosen as the standard and assigned a mass value
36
The masses of all other atoms are expressed in
Relation to this defined standard
37
The standard used by scientists to compare units of atomic mass is the
Carbon-12 atom
38
One atomic mass unit or 1 amu
Is exactly 1/12 the mass of a carbon-12 atom
39
The atomic mass of any other atom is determined by comparing it with the mass of the
Carbon-12 atom
40
Isotopes of an element may occur naturally or they may be
Made in the laboratory (artificial isotopes)
41
Although isotopes have different masses they do not
Differ significantly in their chemical behavior
42
The masses of subatomic particles can also be expressed in the
Atomic mass scale
43
The mass of the electron is
0.000 5486 amu
44
The mass of the proton is
1.007 276 amu
45
The mass of a neutron is
1.008 665 amu.
46
The mass number and relative atomic mass of a given nuclide are
Quite close to each other
47
Mass number and relative atomic mass are not identical because the
Proton and neutron masses deviate slightly from 1 amu and the atomic masses include electrons
48
A small amount of mass is changed to energy in the creation of a
Nucleus from its protons and neutrons
49
The percentage of each isotope in the naturally occurring element on earth is
Nearly always the same no matter where the element is found
50
The percentage at which each of an elements isotopes occurs in nature is taken into account when
Calculating the elements average atomic mass
51
Average atomic mass is the
Weighted average of the atomic masses of the naturally occurring isotopes of an element
52
The average atomic mass of an element depends on both the
Mass and the relative abundance of each of the elements isotopes
53
The average atomic mass of copper can be calculated by
Multiplying the atomic mass of each isotope by its relative abundance (in decimal form) and adding the results
54
Most atomic masses are known to
Four or more significant figures
55
The relative atomic mass scale makes it possible to know
How many atoms of an element are present in a sample of the element with a measurable mass
56
Three very important concepts- mole, Avogadro's number, and molar mass- provide
The basis for relating masses in grams to numbers of atoms
57
A mole is the amount of a
Substance that contains as many particles as there are atoms in exactly 12 g of carbon-12
58
The mole is a
Counting unit
59
The number of particles in a mole has been
Experimentally determined in a number of ways
60
The best modern value for the number of particles in a mole is
6.022 141 79 x 10^23 which means that exactly 12 g of carbon contains that number of carbon-12 atoms
61
The number of particles in a mole is known as
Avogadro's number
62
Avogadro's number is named for the 19th century Italian scientist whose ideas were
Crucial in explaining the relationship between mass and numbers of atoms
63
Avogadro's number is the number of
Particles in exactly one mole of a pure substance
64
For most purposes Avogadro's number is rounded to
6.022 x 10^23
65
An alternative definition of mole is the amount of a substance that cot subs
Avogadro's number of particles
66
The molar mass of a substance is the
Mass of one mole of a pure substance
67
Molar mass is usually written in units of
g/ mol
68
The molar mass of an element is numerically equal to the
Atomic mass of the element in atomic mass u to
69
The molar mass of an element contains
One mole of atoms
70
Chemists use molar mass as a
Conversion factor in chemical calculations
71
Avogadro's number can be used to find the
Number of atoms of an element from the amount in moles or to find the amount of an element in miles from the number of atoms
72
Such problems are useful in demonstrating the
Meaning of Avogadro's number
73
In these calculations Avogadro's number is expressed in
Units of atoms per mole
74
Neon is a
Minor component of the atmosphere