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chemistry > bonding and nomenclature II > Flashcards

bonding and nomenclature II Flashcards

1
Q

what are acids?

A

ionic compounds that contain H^+1 as their cation

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2
Q

how are acids named?

A

based on their anion

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3
Q

how is an anion named if it ends in -ide?

A

hydro__ic acid (the root name of the anion goes in the space)

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4
Q

how is an anion named if it ends in -ate?

A

__ic acid

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5
Q

how is an anion named if it ends in -ite?

A

__ous acid

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6
Q

mnemonic devices to remember -ate and -ite endings:

A

i “ate” something “ic”ky

gingiv”ite”“ous”

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7
Q

prefixes for molecular compounds:

A 
1 - mono
2 - di
3 - tri
4 - tetra
5 - penta
6 - hexa 
7 - hepta
8 - octa
9 - nona
10 - deca
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8
Q

what are the rules for naming molecular compounds?

A
  1. use the prefixes to indicate how many of each element is in one molecule
  2. change the ending on the second element to “-ide”
  3. if there’s only one of the first element, do not write “mono” in front of it
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9
Q

where will atoms in a molecule try to orient themselves? why?

A

as far as possible due to electron density in the bond repelling other electron-dense areas

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10
Q

what does VSEPR stand for? what does it mean? what does it cause?

A

valence shell electron pair repulsion. it means that paired valence electrons push away from each other. it causes the 3D structure of molecules

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11
Q

what is VSEPR based on?

A

the total number of electron domains around the central atom

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12
Q

what is an electron domain?

A

the area where electron pairs are most likely to be found

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13
Q

in what form do pairs of electrons come?

A

single bond, multiple bond, or nonbonding pair

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14
Q

describe all configurations and aspects of configurations with 2 electron domains:

A 
domain geometry: linear
bonding pairs: 2
nonbonding pairs: 0
molecular geometry: linear
bond angle: 180º
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15
Q

describe all configurations and aspects of configurations with 3 electron domains:

A 
domain geometry: trigonal planar
bonding pairs: 3
nonbonding pairs: 0
molecular geometry: trigonal planar
bond angle: 120º
domain geometry: trigonal planar
bonding pairs: 2
nonbonding pairs: 1
molecular geometry: bent
bond angle: <120º
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16
Q

describe all configurations and aspects of configurations with 4 electron domains:

A 
shape: tetrahedral
bonding pairs: 4
nonbonding pairs: 0 
molecular geometry: tetrahedral
bond angle: 109.5º
shape: tetrahedral
bonding pairs: 3
nonbonding pairs: 1
molecular geometry: trigonal pyramidal
bond angle: <109.5º
shape: tetrahedral
bonding pairs: 2
nonbonding pairs: 1
molecular geometry: bent
bond angle: <109.5º
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17
Q

describe all configurations and aspects of configurations with five electron domains:

A

5 and onward break the octet rule

shape: trigonal bipyramidal
bonding pairs: 5
nonbonding pairs: 0
molecular geometry: trigonal bipyramidal
bond angles: 120º, 90º (120 between the arms, 90 between the branches)
shape: trigonal bipyramidal
bonding pairs: 4
nonbonding pairs: 1
molecular geometry: seesaw
bonding angles: 120º, 90º
shape: trigonal bipyramidal
bonding pairs: 3
nonbonding pairs: 2
molecular geometry: t-shaped
bonding angles: 120º, 90º
shape: trigonal bipyramidal
bonding pairs: 2
nonbonding pairs: 3
molecular geometry: linear
bonding angle: 180º
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18
Q

what parts of a molecule with five electron domains become its nonbonding pairs?

A

its three lobes

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19
Q

describe all configurations and aspects of configurations with 6 electron domains

A 
shape: octahedral
bonding pairs: 6
nonbonding pairs: 0
molecular geometry: octahedral
bond angle: 90º
shape: octahedral
bonding pairs: 5
nonbonding pairs: 1
molecular geometry: square pyramidal
bond angle: 90º
shape: octahedral
bonding pairs: 4
nonbonding pairs: 2
molecular geometry: square planar
bond angle: 90º
shape: octahedral
bonding pairs: 3
nonbonding pairs: 3
molecular geometry: t-shaped
bonding angles: 120º, 90º
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20
Q

what parts of a molecule with six electron domains become its nonbonding pairs first?

A

the polars (top and bottom)

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21
Q

when is the only time we deal with 5 and 6 domains for central atoms?

A

when they are able to obtain more than an octet

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21
Q

when is the only time we deal with 5 and 6 domains for central atoms?

A

when they are able to obtain more than an octet

22
Q

how many poles may bonds have? what does it depend on?

A

2, their electronegativites

23
Q

what is a polar bond?

A

bonds where the electrons are shared unequally between atoms

24
Q

which atom in a polar bond pulls the electron closer to itself?

A

the more electronegative atom

25
Q

what is the electronegativity difference between atoms in a polar covalent bond?

A

0.5-1.7, but it can be higher than 1.7

26
Q

what does it mean in terms of polarity when atoms are different?

A

it means that each atom has a different pull on the electrons

27
Q

what is a nonpolar bond?

A

when electrons are shared equally between two atoms

28
Q

what constitutes a nonpolar bond?

A

when atoms that are the same have the same pull on the shared electrons (same electronegativity values) or have an electronegativity difference between 0-0.4

29
Q

what are the general rules to determining if a molecule is polar or nonpolar?

A
  1. different atoms around a central atom will always be polar molecules
  2. same atoms around a central atom are always nonpolar molecules
30
Q

how should you picture unshared electrons/lone pairs when it comes to polarity?

A

picture them as a different atom, making the bond polar regardless of if the central atom is surrounded by the same atoms (eg H2O)

31
Q

what does molecular polarity depend on?

A
  1. bond polarity

2. the shape of the molecule (symmetrical versus asymmetrical)

32
Q

what is a network solid?

A

when many atoms are bonded together to make a large crystal

33
Q

what is a network solid referred to as?

A

a macromolecule

34
Q

what is the structure of a macromolecule?

A

extremely rigid

35
Q

describe the properties of a network solid/macromolecule. why does it have these properties?

A

very strong crystal, very high boiling point/melting point. not due to the type of bond (covalent), but because of how many bonds are present

36
Q

what are examples of network solids?

A

pure c (diamond), SiC (coating for very hard tools), graphite, SiO2 (quartz)

37
Q

what do metals not do well? what does this lead to when metal atoms are bonded together?

A

metals don’t hold electrons very well, leading to electrons moving between valence shells when metals are bonded and not staying around any particular atoms (they instead “float” from atom to atom)

38
Q

what is it called when in a metallic bond electrons move between valence shells, “floating” from atom to atom?

A

the “sea of mobile electrons”

39
Q

what properties does mobility give to metals?

A

malleability, conductivity, and luster

40
Q

what is a metallic bond

A

metal + metal

41
Q

what is an alloy?

A

different metal atoms bonded together

42
Q

what is brass?

A

copper + zinc

43
Q

what is an ionic bond made of? what are its properties with regards to the periodic table, electronegativity, and ionic character?

A

metal + nonmetal, further apart on the periodic table, greater difference in electronegativity, higher ionic character

44
Q

which elements have high ionic characters? which have higher ionic characters?

A

Cr, P = high ionic character

Cl, Ca = higher ionic character

45
Q

what is a covalent bond comprised of? how large is its difference in electronegativity?

A

nonmetal + nonmetal, small difference in electronegativity

46
Q

what is a ternary substance? what type of bond is a bond between a polyatomic ion and an atom?

A

a compound containing a polyatomic ion, which is an ion that is covalently bonded together. ionic.

47
Q

what makes a substance conduct electricity?

A

if it has freely moving charged particles (ions, electrons, etc., as long as they can move)

48
Q

in what form do metals conduct electricity? what allows electricity to flow in metals?

A

solid or liquid form, freely moving electrons

49
Q

in what form do ionic substances not conduct electricity? why?

A

solid form, since ions are locked in place; they have charges but aren’t freely moving

50
Q

in what state can ionic substances conduct electricity?

A

liquid; when melted, they can conduct electricity since ions are hot enough to move past each other

51
Q

what happens to ions in a solutions? what does this allow? why?

A

in a solution, ions separate, making them free to move and allowing them to conduct electricity

52
Q

describe covalent conductivity as a solid, liquid, or in a solution, and explain why each is the case

A

solid - doesn’t conduct electricity, no charged particles
liquid - doesn’t conduct electricity, no charged particles
solution - some types of covalent molecules can be broken down to make ions

53
Q

describe conductivity in ionization

A

conducts some electricity, because only a few of the molecules in the sample are broken down

chemistry (2 decks)

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