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Chem > Ch 6 Section 2 > Flashcards

Ch 6 Section 2 Flashcards

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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
Q

In forming a covalent bond the hydrogen atoms release energy as they

A

Change from isolated individual atoms to parts of a molecule

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26
Q

The amount of energy released equals the difference between the

A

Potential energy at the zero level (separated atoms) and that at the bottom valley (bonded atoms)

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27
Q

The same amount of energy must be added to separate the

A

Bonded atoms

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28
Q

Bond energy is the energy required to

A

Break a chemical bond and form neutral isolated atoms

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29
Q

Scientists usually report bond energies in kilojoules per mole (kJ/mol) which indicates the

A

Energy required to break one mile of bonds in isolated molecules

30
Q

Bond lengths and bond energies vary with the types of

A

Atoms that have combined

31
Q

Even the energy of a bond between the same two types of atoms

A

Varies somewhat depending on what other bonds the atoms have formed

32
Q

All individual hydrogen atoms contain a single unpaired electron in a

A

1s atomic orbital

33
Q

When two hydrogen atoms form a molecule they share

A

Electrons in a covalent bond

34
Q

Sharing electrons for hydrogen atoms allows each atom to have

A

The stable electron configuration of helium

35
Q

The tendency for atoms to achieve noble gas configurations my bonding covalently extends beyond the

A

Simple case of a hydrogen molecule

36
Q

Unlike other atoms the noble gas atoms exist

A

Independently in nature

37
Q

Noble gas atoms possess a minimum of energy existing on their own because of the

A

Special stability of their electron configurations

38
Q

Other main group atoms can effectively fill their outermost s and p orbitals with electrons by

A

Sharing electrons through covalent bonding

39
Q

Such bond formation follows the

A

Octet rule

40
Q

Octet rule: chemical compounds tend to form so that each atom by gaining losing or sharing electrons has an

A

Octet of electrons in its highest occupied energy level

41
Q

Most main group elements tend to form covalent bonds according to the

A

Octet rule

42
Q

Because electron pairs are shared in covalent bonds boron tends to form bonds in which

A

It is surrounded by six electrons

43
Q

Other elements can be surrounded by more than with electrons when they

A

Combine with the highly electronegative elements fluorine, oxygen, and chlorine

44
Q

In these cases of expanded valence bonding involves electrons in

A

D orbitals as well as in s and p orbitals

45
Q

Covalent bond formation usually involves only the electrons in an atoms

A

Outermost energy levels, the atoms valence electrons

46
Q

Electron for notation is an electron configuration notation in which

A

Only the valence electrons of an atom of a particular element are shown indicates by dots places around the elements symbol

47
Q

In electron dot notation the inner shell electrons

A

Are not shown

48
Q

In general an elements number of valence electrons can be determined by adding the

A

Superscripted of the elements noble gas notation

49
Q

The pair of dots between the two symbols represents the

A

Shared pair of a covalent bond

50
Q

An unpaired pair (lone pair) is a pair of electrons that is not

A

Involved in bonding and that belongs exclusively to one atom

51
Q

The pair of dots representing a shared pair of electrons in a covalent bond is often replaced by a

A

Long dash

52
Q

Lewis structures: formulas in which atomic symbols represent

A

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
Q

It is common to write Lewis structures that show only the

A

Electrons that are shared, using dashes to represent the bonds

54
Q

A structural formula indicated the

A

Kind number arrangement and bonds but not the unshared pairs of the atoms in a molecule

55
Q

The Lewis structures for many molecules can be drawn if one knows the

A

Composition of the molecule and which atoms are bonded to each other

56
Q

A single covalent bond (single bond) is a covalent bond in which

A

One pair of electrons is shared between 2 atoms

57
Q

Atoms of some elements can share

A

More than one electron pair

58
Q

A double covalent.bond (double bond) is a covalent bond in which

A

2 pairs of electrons are shared between 2 atoms

59
Q

A double bind is shown either by two

A

Side by side pairs of dots or by two parallel dashes

60
Q

All four electrons in a double bond belong to

A

Both atoms

61
Q

A triple bond is a covalent bond in which

A

3 pairs of electrons are shared between two atoms

62
Q

Multiple bonds

A

Double and triple bonds

63
Q

Double bonds in general have greater

A

Bond energies and are shorter than single bonds

64
Q

Triple bonds are even

A

Stronger and shorter

65
Q

In writing Lewis structures for molecules that contain carbon nitrogen or oxygen one must remember that

A

Multiple bonds between pairs of these atoms are possible

66
Q

A hydrogen atom always forms a

A

Single covalent bond

67
Q

The need for a multiple bond becomes obvious if there are not enough

A

Valence electrons to complete octets by adding unshared electrons

68
Q

Some molecules and ions cannot be represented

A

Adequately by a single Lewis structure

69
Q

Resonance refers to bonding in

A

Molecules or ions that cannot be correctly represented by a single Lewis structure

70
Q

To indicate resonance a double headed arrow is

A

Placed between a molecules resonance structures

71
Q

There are many covalently bonded compounds that do not contain individual molecules but instead can be pictures as

A

Continuous 3 dimensional networks of bonded atoms

72
Q

Many chemical compounds including most of the chemicals that are in living things and are produced by living things are composed of

A

Molecules

Chem (54 decks)

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