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Chem 101 > bonds > Flashcards

bonds Flashcards

1
Q

what are covalent bonds between

A

nonmetal and nonmetal

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1
Q

how are covalent bonds formed

A

through sharing electrons

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2
Q

how are ionic bonds formed

A

through transferring electrons

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3
Q

what are ionic bonds between

A

nonmetal and metal

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4
Q

what is a polar covalent bond

A

a bod where one end gets more electrons than the other

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5
Q

which side of a polar covalent bond is negatively charged

A

the side with more electrons (greater electron density)

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6
Q

which side of a polar covalent bond is positively charged

A

the side with less electrons

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7
Q

what is electronegativity

A

the ability of an atom to attract bonding electrons to itself

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8
Q

what happens to electronegativity as you go across the period

A

it increases

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9
Q

what happens to electronegativity as you go down the group

A

it decreases

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10
Q

what is a pure covalent

A

where the difference in electronegativity between bonded atoms is 0; there is equal sharing of atoms

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11
Q

what type of bond is it if electronegativity difference is between 0.1 - 0.4

A

nonpolar covalent

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12
Q

what type of bond is it if electronegativity difference is between 0.5 - 1.9

A

polar covalent

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13
Q

what type of bond is it if electronegativity difference is at least 2.0

A

ionic

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14
Q

what type of bond is it if electronegativity difference is = 0

A

pure covalent

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15
Q

how to find polarity of bond

A

look at how far the elements in the bond are from each other on periodic table; if they are further from each other, they will have a greater electronegativity difference and will be more polar

16
Q

if elements in a bond are far away from each other on periodic table; what is their polarity

A

increased polarity; increased electronegativity difference

17
Q

if elements in a bond are close to each other on periodic table; what is their polarity

A

less polarity; less electronegativity difference

18
Q

what are bonding pairs

A

Electrons that are shared by atoms

19
Q

what are lone pairs

A

electrons that are not shared by atoms, but rather belong to only one of the particular atoms

20
Q

what is a single covalent bond

A

When two atoms share one pair of electrons

21
Q

what is a double covalent bond

A

When two atoms share two pairs of electrons

22
Q

what is a triple covalent bond

A

When two atoms share three pairs of electrons

23
Q

polar bond definition

A

two different elements with significant electronegativity difference between them

24
Q

What is a resonance structure

A

a set of two or more Lewis Structures that collectively describe the electronic bonding of a single polyatomic species including fractional bonds and fractional charges

25
Q

can resonance structures have different numbers of electrons?

A

No

26
Q

What do better resonance structures have?

A

fewer formal charges; smaller formal charges; negative formal charge on the more electronegative atom

27
Q

what must formal charge of an ion add up to

A

the charge of the ion

28
Q

what must the formal charge of a neutrally charged molecule add up to

A

zero

29
Q

what is formula to find formal charge

A

(# of valence electrons) - [ (# of nonbonding electrons) + (½ x # of bonding electrons) ]

30
Q

what happens to bond strength as you go down a column

A

the bonds get weaker

31
Q

what happens to bond strength as you go across the period

A

the bonds get stronger

32
Q

the shorter the covalent bond, the _______ the bond

A

stronger

33
Q

the more electrons two atoms share, the _________ the covalent bond

A

stronger

34
Q

how is bond strength measured

A

bond strength is measured by how much energy must be added into the bond to break it in half

35
Q

how is bond length measured

A

Bond length is determined by measuring the distance between the nuclei of bonded atoms

Chem 101 (13 decks)

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