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Honors Chemistry > Chapter 6 Covalent Bonding > Flashcards

Chapter 6 Covalent Bonding Flashcards

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1
Q

What is the name of N2O3?

A

Dinitrogen trioxide

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2
Q

What is the chemical formula for tetrasulfur pentoxide?

A

S4O5

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3
Q

What is the name of C3Cl8

A

Tricarbon octachloride

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4
Q

What is the chemical formula for Nitrogen triiodide?

A

NI3

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5
Q

What is the name of Br6F10 ?

A

Hexabromine decafluoride

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6
Q

What is the chemical formula for Tetraphosphorous Pentachloride ?

A

P4Cl5

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7
Q

What is the name of CO

A

carbon monoxide

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8
Q

What is the chemical formula for Fluorine trisulfide ?

A

FS3

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9
Q

What is the name of S2Br6?

A

Disulfur hexabromide

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10
Q

What is the chemical formula for phosphorus triiodide?

A

PI3

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11
Q

What is the chemical formula for chlorine pentoxide?

A

ClO5

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12
Q

What is the name of P4S5?

A

Tetraphosphorus pentasulfide

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13
Q

What is the name of SeF3?

A

selenium trifluoride

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14
Q

What is the prefix for 1?

A

mono

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15
Q

What is the prefix for 8?

A

octa

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16
Q

What is the prefix for 10?

A

deca

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17
Q

What is the prefix for 4?

A

tetra

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18
Q

covalent compounds contain:

A

2 nonmetals

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19
Q

What is the correct name for C4H6?

A

tetracarbon hexahydride

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20
Q

NH3 has how many lone pairs?

A

1

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21
Q

What is a covalent bond?

A

A bond formed when two atoms share a pair of electrons

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22
Q

In chemical compounds, covalent bonds form when

A

pairs of electrons are shared between two non-metal atoms.

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23
Q

The melting point of sugar is__________________ the melting point of table salt.

A

less than

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24
Q

What are properties of a covalently-bonded compound?

A

Low melting point, Generally insoluble/immiscible in water, Generally soft and flexible

25
Q

How does the covalent bond form between two atoms?

A

When the two atoms share electrons

26
Q

Why is the H2 molecule more stable than two separate hydrogen atoms?

A

Hydrogen only needs two electrons to become stable so when separate hydrogen atoms share their single electrons, it becomes stable

27
Q

Explain why the stability described in item 2 does or does not hold true for most covalent bonds?

A

The H2 molecule is stable but not true for other bonds because each e- has to have 8 valence electrons except H

28
Q

How does a covalent bond differ from an ionic bond

A

Covalent bonds share electrons, ionic bonds transfer electrons from one another

29
Q

What is a molecular orbital?

A

a regions of high probability that is occupied by in individual electron as it travels around two or more associated nuclei

30
Q

Describe the potential energy change that occurs when two hydrogen atoms approach each other and form a covalent bond

A

The potential energy of two separate hydrogen atoms (right) decreases as they approach each other, and the single electrons on each atom are shared to form a covalent bond.

31
Q

In terms of energy, why is the H-H bond stable?

A

It is stable because of the shared electrons. Hydrogen only needs two electrons to become stable

32
Q

What is bond length?

A

The average distance between two bonded atoms at their minimum potential energy

33
Q

What is bond energy?

A

the energy required to break the chemical bond between two atoms and separate them

34
Q

The tendency of an atom to attract bonding electrons to itself when it bonds with another atom is called ______________

A

electronegativity

35
Q

_____________is an attraction between two atoms in which electrons are shared equally between atoms.

A

nonpolar covalent

36
Q

____________is an attraction between two atoms in which bonding electrons are localized on the more electronegative atom.

A

polar covalent

37
Q

__________ is a molecule in which one end has a partial positive charge and the opposite end has a partial negative charge.

A

dipole

38
Q

In general, if the difference in electronegativity between two atoms is between 0 and 0.4, the bond is __________.

A

nonpolar covalent

39
Q

If the electronegativity difference between two atoms is between 0.5 and 1.7, the bond formed is __________.

A

polar covalent

40
Q

If the electronegativity difference between two atoms is greater than 2.1 the bond formed is __________.

A

ionic

41
Q

A possible Lewis structure of a molecule for which more than one Lewis structure can be written is called a __________ structure

A

resonance

42
Q

A structure in which atomic symbols represent nuclei and inner-shell electrons and in which dots are used to represent valence electrons is called a ________ structure.

A

Lewis

43
Q

explain the difference between single double and triple bonds

A

A single bond is formed when two atoms share one pair of electrons, whereas a double bond is formed when two atoms share two pairs (four electrons). Three pairs of electrons (six atoms) are shared to form triple bonds.

44
Q

What does the VSEPR theory predict?

A

The arrangement of electron pairs around each central atom and the correct arrangement of atoms in a molecule.

45
Q

How does one unbonded pair of electrons affect the shape of a molecule?

A

The electrons in the unbonded pair repel bonding electrons as far away from it as possible.

46
Q

How do multiple unbonded pairs of electrons affect the shape of a molecule?

A

They can repel each other as well as bonding electrons, forming a bent molecule.

47
Q

What evidence is there to support the idea that opposite polar ends of molecules attract each other?

A

The energy required to separate polar molecules is greater than that required to separate non polar molecules.

48
Q

How do polarity and shape of molecules relate to the properties of a substance?

A

They can affect how a molecule fits into another structure and how it tastes. It can also affect how easy the molecule is to separate and its attraction to positively or negatively charged objects.

49
Q

Why is bond length an average rather than a fixed number?

A

Because bonded atoms can experience vibration causing the bond to stretch and bend.

50
Q

Electron affinity is:

A

energy change when an electron is acquired by a neutral atom

51
Q

Covalent bonds have a ______ boiling point

A

low

52
Q

What does the Lewis structure help us see?

A

The arrangement of electrons in a a molecule

53
Q

As the number of bonds increases in a molecule, the bond length:

A

decreases

54
Q

Trigonal planar angle:

A

120

55
Q

Bent angle with one lone pair:

A

116

56
Q

Tetrahedral angle:

A

109.5

57
Q

Trigonal pyramidal angle:

A

107

58
Q

Bent angle with two lone pairs:

A

105

Honors Chemistry (23 decks)

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