Ch 6 Section 2 Flashcards

1
Q

A molecule is a neutral group of

A

Atoms that are held together by covalent bonds

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2
Q

A single molecule of a chemical compound is an individual unit capable of

A

Existing on its own

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3
Q

Molecules may consist of two or more

A

Atoms of the same element or two or more different atoms

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4
Q

Molecular compound is a chemical compound whose

A

Simplest units are molecules

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5
Q

The composition of a compound is given by

A

It’s chemical formula

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6
Q

A chemical formula indicated the relative numbers of

A

Atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts

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7
Q

The chemical compound of a molecular compound is referred to as a

A

Molecular formula

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8
Q

A molecular formula shows the types and numbers of

A

Atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts

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9
Q

The molecular formula for water reflects the fact that a single water molecule consists of

A

One oxygen atom joined by separate covalent bonds to two hydrogen atoms

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10
Q

A molecule of oxygen O2 is an example of

A

A diatomic molecule

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11
Q

A diatomic molecule is a molecule containing

A

Only 2 atoms

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12
Q

The approaching nuclei and electrons are

A

Attracted to each other

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13
Q

The attraction between nuclei and electrons corresponds to a decrease in

A

The total potential energy of the atoms

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14
Q

The two nuclei repel each other and the two electrons

A

Repel each other which results in an increase in Potential energy

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15
Q

Relative strength of attraction and repulsion between the charged particles depends on the

A

Distance separating the atoms

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16
Q

When the atoms first sense each other the electron proton attraction is stronger than the

A

Electron electron and proton proton repulsions

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17
Q

The atoms are drawn to each other and their

A

Potential energy is lowered

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18
Q

The attractive force continues to dominate and the total potential energy continues to

A

Decrease until a distance is reached at which the repulsion between the like charges equals the attraction of the opposite charges

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19
Q

When a distance is reached at which the repulsion between like charges equals the attraction of the opposite charges the potential energy is at a

A

Minimum and a stable hydrogen molecule forms (in the case of a hydrogen-hydrogen bond)

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20
Q

A closer approach of the atoms results in a sharp rise in potential energy as

A

Repulsion becomes increasingly greater than attraction

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21
Q

The bottom of the valley in the curve represents the

A

Balance between attraction and repulsion in a stable covalent bond

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22
Q

The molecules electrons can be pictured as

A

Occupying overlapping orbitals moving about freely in either orbital

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23
Q

The bonded atoms vibrate a bit but as long as their potential energy remains close to the minimum they are

A

Covalently bonded to each other

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24
Q

The distance between two bonded atoms at their minimum potential energy is the

A

Bond length

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25
In forming a covalent bond the hydrogen atoms release energy as they
Change from isolated individual atoms to parts of a molecule
26
The amount of energy released equals the difference between the
Potential energy at the zero level (separated atoms) and that at the bottom valley (bonded atoms)
27
The same amount of energy must be added to separate the
Bonded atoms
28
Bond energy is the energy required to
Break a chemical bond and form neutral isolated atoms
29
Scientists usually report bond energies in kilojoules per mole (kJ/mol) which indicates the
Energy required to break one mile of bonds in isolated molecules
30
Bond lengths and bond energies vary with the types of
Atoms that have combined
31
Even the energy of a bond between the same two types of atoms
Varies somewhat depending on what other bonds the atoms have formed
32
All individual hydrogen atoms contain a single unpaired electron in a
1s atomic orbital
33
When two hydrogen atoms form a molecule they share
Electrons in a covalent bond
34
Sharing electrons for hydrogen atoms allows each atom to have
The stable electron configuration of helium
35
The tendency for atoms to achieve noble gas configurations my bonding covalently extends beyond the
Simple case of a hydrogen molecule
36
Unlike other atoms the noble gas atoms exist
Independently in nature
37
Noble gas atoms possess a minimum of energy existing on their own because of the
Special stability of their electron configurations
38
Other main group atoms can effectively fill their outermost s and p orbitals with electrons by
Sharing electrons through covalent bonding
39
Such bond formation follows the
Octet rule
40
Octet rule: chemical compounds tend to form so that each atom by gaining losing or sharing electrons has an
Octet of electrons in its highest occupied energy level
41
Most main group elements tend to form covalent bonds according to the
Octet rule
42
Because electron pairs are shared in covalent bonds boron tends to form bonds in which
It is surrounded by six electrons
43
Other elements can be surrounded by more than with electrons when they
Combine with the highly electronegative elements fluorine, oxygen, and chlorine
44
In these cases of expanded valence bonding involves electrons in
D orbitals as well as in s and p orbitals
45
Covalent bond formation usually involves only the electrons in an atoms
Outermost energy levels, the atoms valence electrons
46
Electron for notation is an electron configuration notation in which
Only the valence electrons of an atom of a particular element are shown indicates by dots places around the elements symbol
47
In electron dot notation the inner shell electrons
Are not shown
48
In general an elements number of valence electrons can be determined by adding the
Superscripted of the elements noble gas notation
49
The pair of dots between the two symbols represents the
Shared pair of a covalent bond
50
An unpaired pair (lone pair) is a pair of electrons that is not
Involved in bonding and that belongs exclusively to one atom
51
The pair of dots representing a shared pair of electrons in a covalent bond is often replaced by a
Long dash
52
Lewis structures: formulas in which atomic symbols represent
Nuclei and inner shell electrons, for pairs or dashes between two atomic symbols represent electron pairs in covalent bonds, and dots adjacent to only one atomic symbols represent unshared electrons
53
It is common to write Lewis structures that show only the
Electrons that are shared, using dashes to represent the bonds
54
A structural formula indicated the
Kind number arrangement and bonds but not the unshared pairs of the atoms in a molecule
55
The Lewis structures for many molecules can be drawn if one knows the
Composition of the molecule and which atoms are bonded to each other
56
A single covalent bond (single bond) is a covalent bond in which
One pair of electrons is shared between 2 atoms
57
Atoms of some elements can share
More than one electron pair
58
A double covalent.bond (double bond) is a covalent bond in which
2 pairs of electrons are shared between 2 atoms
59
A double bind is shown either by two
Side by side pairs of dots or by two parallel dashes
60
All four electrons in a double bond belong to
Both atoms
61
A triple bond is a covalent bond in which
3 pairs of electrons are shared between two atoms
62
Multiple bonds
Double and triple bonds
63
Double bonds in general have greater
Bond energies and are shorter than single bonds
64
Triple bonds are even
Stronger and shorter
65
In writing Lewis structures for molecules that contain carbon nitrogen or oxygen one must remember that
Multiple bonds between pairs of these atoms are possible
66
A hydrogen atom always forms a
Single covalent bond
67
The need for a multiple bond becomes obvious if there are not enough
Valence electrons to complete octets by adding unshared electrons
68
Some molecules and ions cannot be represented
Adequately by a single Lewis structure
69
Resonance refers to bonding in
Molecules or ions that cannot be correctly represented by a single Lewis structure
70
To indicate resonance a double headed arrow is
Placed between a molecules resonance structures
71
There are many covalently bonded compounds that do not contain individual molecules but instead can be pictures as
Continuous 3 dimensional networks of bonded atoms
72
Many chemical compounds including most of the chemicals that are in living things and are produced by living things are composed of
Molecules