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chemisty > chem struc & bonding > Flashcards

chem struc & bonding Flashcards

1
Q

ionic bond def: __________________________ forces of __________________ between _____________ charged ______ in a _____________________ structure

A

strong electrostatic, attraction, oppositely, ions, giant ionic lattice

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2
Q

ionic bond def:

A

strong electrostatic forces of attractions between oppositely charged ions in a giant ionic lattice structure

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3
Q

ionic bonds are usually between

A

metal & non-metal

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4
Q

in same period, size of cation is always __________ than size of anion (cus cations ______ electrons & anions ______ electrons)

A

smaller, lose, gain

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5
Q

ionic compounds have

A

giant ionic lattice struc

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6
Q

when ions come tgt, they arrange themselves in a continuous 3d lattice of _____________cation and anions, which _____________ attractive forces between _____________ charged ions & ____________ repulsion between ____________ charged ions

A

alternating, maximises, oppositely, minimises, similarly

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7
Q

ionic bonds are generally ________ and a _______ amt of energy is needed to break such bonds

A

strong, large

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8
Q

the ____________ the charges of ion, the _____________ the ionic bonds

A

greater, stronger

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9
Q

the ___________ the ionic radius, the ___________ the ionic bonds

A

smaller, stronger

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10
Q

ionic radius for cations & anions ____________ across period (cus no. of protons increase –> __________ pull to nucleus) & ____________ down grp (no. of electron shells)

A

decreases, stronger, increases

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11
Q

IMPT: how to ans qns with reference to structure & bonding: which ionic compound have stronger ionic bonds
1. do they have giant ionic lattice?
2. compare cation & anion charges (__________ charge, _________ bonds)
3. compare ionic radii of cation & anion (___________ radii, ____________ bonds)
4. hence, ………. is stronger as _______ energy is needed to ______________ the __________ ionic bond

A

greater, stronger
smaller, stronger
more, overcome, stronger

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12
Q

more protons –> ___________ electrostatic forces of attraction –> shell shrinks –> _________ to nucleus –> radii ____________

A

greater, closer, smaller

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13
Q

with reference to structure & bonding, predict if …… has a higher/lower boiling point than …….

A
  1. compare both lattice structures (ionic/not)
    2.compare charges (greater charges stronger bonds)
  2. compare ionic radii (smaller radii, stronger bonds)
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14
Q

ionic compounds hav high boiling & melting pts bc a _________ amt of energy is needed to _____________ the _________ electrostatic forces of _________________ between opp. charged ions

A

large, overcome, strong, attraction

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15
Q

ionic compounds r gd conductors of electricity in MOLTEN & AQUEOUS states but non-conductors in SOLID state as in the molten/aqueous state, there are _______ mobile ions to act as _______________________________ to conduct electricity, but in solid state ions can only ___________ abt their_______ positions–> no ______________________________ to conduct electricity

A

free, mobile charge carriers, vibrate, fixed, free mobile ions

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16
Q

ionic compounds r generally soluble in __________ but insoluble in _____________ ___________ such as oil and turpentine

A

water, organic solvents

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17
Q

ionic compounds r hard cos in an ionic _______, opp. charged ions r held tgt by ________ ____________________ ________ of attraction

A

solid, strong electrostatic forces

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18
Q

ionic compounds r brittle cos when stress is applied on an ionic _________, it causes _________ of layers of ions, making ions of __________ charges to come tgt, & resultant _____________ __________ the ionic structure

A

lattice, sliding, similar, repulsion shatters

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19
Q

ionic compounds r used in refractories as they can withstand _______ temps

A

high

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20
Q

metallic bonds r formed when metal _______ ______ valence electrons to from _________. these valence electrons are ______________

A

atoms lose, cations, delocalised

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21
Q

metallic bonds def: metallic bonds are _________ _______________ __________ of attraction between metal __________ & the _______ of _________________ electrons in a __________ ______________ lattice

A

strong electrostatic forces, cations, sea of delocalised, giant metallic

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22
Q

metallic bonds def: metallic bonds are

A

strong electrostatic forces of attraction between metal cations and sea of delocalised electrons in a giant metallic lattice

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23
Q

delocalised electrons are capable of ____________ _________ between the metal cations

A

moving freely

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24
Q

metals hav __________ _____________ structure

A

giant metallic

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25
Q

metallic bonds are generally _________ & _________ amt of energy is needed to break them

A

strong, large

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26
Q

the ____________ the no. of valence electrons contributed to sea of ________________ electrons per _______, the _____________ the ____________ bonds (eg metallic bond in magnesium is stronger than sodium cos mg has 2 valence electrons per atom compared to 1 per sodium atom)

A

greater, delocalised, atom, stronger, metallic

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27
Q

the larger the ____________ radius, the ____________ the _____________ bonds (cos delocalised electrons less strongly held by nuclei cus it’s furthest away-> attraction between electrons & cations weaker)

A

metallic, weaker, metallic

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28
Q

ionic radius for cations & anions decreases ___________ ___________ & increases _________ _________

A

across period, down group

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29
Q

metals have high boiling & melting pts. bc _________ amt of energy is needed to overcome _________ ____________________ _________ of attraction between metal __________ & _______ of ____________________ ______________

A

large, strong electrostatic forces, cations, sea, delocalised electrons

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30
Q

metals are gd conductors of electricity cos there’s a ______________ of ________________ ________________ to act as mobile charge ___________ to conduct electricity

A

presence, delocalised electrons, carriers

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31
Q

metals r gd thermal conductors: when heat applied to 1 end of metal, ____________ energy of the _______________ at that end increases & the energy is transferred throughout rest of metal by the ________________ electrons to ________ parts of metal

A

kinetic, electrons, delocalised, other

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32
Q

metals are malleable & ductile bc when force is applied, the __________ of ________ can easily __________ _______ each other w/o breaking the metallic bond; the metallic bonds are easily ________________ & the __________________________ lattice is restored

A

layers, atoms, slide over, reformed, giant metallic

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33
Q

malleable def: ability to be _______________/____________ ______ sheets w/o cracking

A

hammered, pressed into

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34
Q

ductile def: ability to be _____________________ into a _______________________

A

drawn out, thin wire

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35
Q

def of alloys: a ___________ of a metal & another ______________(usually metals)

A

mixture, element

36
Q

def of alloys:

A

a mixture of a metal and another element

37
Q

alloys are much ____________ & __________ than _______ metals, cos the arrangement of atoms is ________________ by the insertion of atoms of a slightly _____ size –> __________________ in structure prevents rows of atoms from _________ over each other

A

stronger, harder, pure, disrupted, diff, irregularity, sliding

38
Q

formation of covalent bonds involves __________ of _______________ between ______ to form a ______________

A

sharing, electrons, atoms, molecule

39
Q

def: covalent bond is the ________________ __________ of _______________ between the ________ _______ of electrons and the _____________ ___________ _______ of both _____ in the bond

A

electrostatic forces, attraction, shared pair, positively charged nuclei, atoms

40
Q

lone pair refers to _____________ _____ _____________ in covalent bonding

A

electrons not involved

41
Q

strength of covalent bond depends on extent of _____________ ____________

A

orbital overlap

42
Q

more effective the orbital overlap, ____________ the covalent bond

A

stronger

43
Q

covalent bonds are _________ and a ________ amt of ___________ is needed to break such bonds

A

strong, large, energy

44
Q

bond length: distance (in nm) between the 2 _______ in a covalent bond

A

nuclei

45
Q

shorter the bond length, ____________ the bond

A

stronger

46
Q

greater the bond energy, ____________ the bond

A

stronger

47
Q

generally, bond strength: trip bond __ double bond __ single bond

A

> ,>

48
Q

ANS SKILL: which covalent bond is stronger
1. atomic radius of the 2 atoms (___________ ->stronger)
2. more effective ____________ ____________ between xx atoms
3. hence leading to ___________ covalent bond

A
  • smaller
  • orbital overlap
  • stronger
49
Q

egs of GIANT MOLECULAR STRUCTURES:

A
  • diamond
  • graphite
  • silicon
  • silicon dioxide
50
Q

egs of SIMPLE MOLECULAR STRUCTURE:

A

H2, N2, H2O, NH3

51
Q

structure of diamond (C), silicon dioxide (SiO2), and silicon (Si): diamond has a _________ _____________ structure where each __________ atom is joined by strong _____________ bonds to ______ other atoms in a _______________ arrangement

A

giant molecular, carbon, covalent, four, tetrahedral

52
Q

allotrope def: _______ forms of the _________ _______________ with _______________ chemical properties but ________ physical properties

A

diff, same element, similar, diff

53
Q

diamond is an _____________ of carbon

A

allotrope

54
Q

diamond has ______________ strong _______________ bonds between _______ resulting in a giant _____ molecular structure

A

numerous, covalent, atoms, 3D

55
Q

diamond has a very _______ ___________ ______ cos a ______ _________ amt of energy is needed to __________________ the _____________ __________ ______________ bonds between ________

A

high melting pt, very large, overcome, numerous strong covalent, atoms

56
Q

diamond is hard cos of the ___________________________________________ between atoms

A

numerous strong covalent bonds

57
Q

diamond is a non-conductor of electricity cos of the _____________ of __________________ _______________ and ________ mobile _______ to conduct electricity ( all the electrons used in covalent bonding)

A

absence, delocalised electrons, free, ions

58
Q

diamonds are _______________ in water

A

insoluble

59
Q

diamonds used as abrasives due to ________ melting points and _____________ (eg diamond tipped tools for cutting)

A

high, hardness

60
Q

silicon (Si) has a similar structure to diamond-> _____________ ______________ properties as diamond

A

similar physical

61
Q

silicon dioxide consists of each silicon atom covalently bonded to ____ ____________ atoms in a _______________ structure and each ___________ atom covalently bonded to ____ silicon atoms

A

4 oxygen, tetrahedral, oxygen, 2

62
Q

silicon dioxide’s phys properties resemble those of diamond:

A
  • hard
  • high melting & boiling pts
  • non-electrical conductor
  • insoluble in water
63
Q

graphite is a __________________________, ______________ structure

A

giant molecular, layered

64
Q

graphite: adjacent layer held tgt by ______ intermolecular forces (dotted lines)

A

weak

65
Q

Graphite: in each layer, each carbon atom is ________________ _________ to _____ other atoms

A

covalently bonded, 3

66
Q

graphite is another _______________ of carbon

A

allotrope

67
Q

Graphite: carbon _______ r arranged in _______________ flat __________ layers

A

atoms, hexagonal, parallel

68
Q

graphite has _________ melting point cos a ____________________ amt of energy is needed to overcome the ________________________________________ between atoms

A

high, very large, numerous strong covalent bonds

69
Q

graphite is ______________________________ parallel to layers but ___________________ perpendicular to layers
cos only ______ valence electrons of each C atom is used for bonding-> 4th non-bonding electron is _____________________ over whole layer & able to act as ________________ charge carriers

A

gd electrical conductor, non-conductor, 3/4, delocalised, mobile

70
Q

graphite is soft & slippery cos the adjacent __________ r held by _____________________________ forces which are _________ overcome -> layers slide over each other _________

A

layers, weak intermolecular, easily, easily

71
Q

graphite is ______________ in water

A

insoluble

72
Q

graphite used as ____________ (eg used in hot machines to reduce friction)

A

lubricant

73
Q

iodine has a ____________ molecular structure

A

simple

74
Q

PHYSICAL properties of simple molecular substances
_____ melting & boiling pt cus ________ amt of energy needed to overcome _________________________ forces of attraction between molecules

A

low, small, weak intermolecular

75
Q

iodine atoms r bonded by __________ covalent bonds within each ______________ but separate ______________ r attracted by _______ intermolecular forces of attraction

A

strong, molecule, molecules, weak

76
Q

PHYSICAL properties of simple molecular substances
__________________ of electricity cos there’s an ______________ of __________________________& ________________________ to conduct electricity

A

non-conductor, absence, free mobile ions, delocalised electrons

77
Q

PHYSICAL properties of simple molecular substances
____________ in water, but soluble in _______________________ (eg benzene)

A

insoluble, organic solvents

78
Q

ANS SKILL: BOILING PT OF SIMPLE VS GIANT MOLECULAR SUBSTANCE
1. x has a lower boiling point than y
2. x has a ________ molecular structure with ________ intermolecular forces of attraction between x molecules
3. y has _________ molecular structure with ____________________________ covalent bonds between y ________
4. _________ energy is needed to ________________ the ____________________________________ bonds in y than the ___________________________ forces of attraction between x molecules

A
  1. simple, weak
  2. giant, numerous strong, atoms
  3. more, overcome, numerous strong covalent, weak intermolecular
79
Q

ANS SKILL: COMPARING BOILING PT OF SIMPLE MOLECULAR SUBSTANCES
1. x has much higher boiling point than y
2. both x & y have ___________ molecular structures with ________ intermolecular forces of _______________
3. x has __________ electron cloud (region of electrons arnd a molecule/atom)-> ____________ & more ________________ intermolecular forces of attraction which needs __________ energy to overcome

A
  1. simple, weak, attraction
  2. larger, stronger, extensive, more
80
Q

electron cloud refers to

A

region of electrons arnd molecule/atom

81
Q

larger the Mr –> __________ the electron cloud –>___________ & more _______________ ___________________ forces of attraction

A

larger, stronger, extensive, intermolecular

82
Q

ANS SKILL: IONIC VS COVALENT COMPOUND MELTING PT
1. state _____________ of each compound (what is giant _________ structure, what is __________ molecular structure
2. the strong _________ bonds in xx needs a ________ amt of energy to overcome it -> _________ melting pt
3. a small amt of energy is needed to overcome the ____________________________________________ between yy molecules -> _______ melting pt

A
  • structure, ionic, simple
  • ionic, large, high
  • weak intermolecular forces of attraction, low
83
Q

some molecules (like water) have a type of intermolecular force of attraction called ________________ bonds

A

hydrogen

84
Q

hydrogen bonds r generally __________ than other ____________________ forces of attraction, but they’re still weaker than ___________, ____________ or __________ bonds

A

stronger, intermolecular, covalent, metallic, ionic

85
Q

hydrogen bonds r between

A

H and O atom (H connect to O)

chemisty (6 decks)

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