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Chemistry Units 1/2 > bonding > Flashcards

bonding Flashcards

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1
Q

metalic bonding

A

a lattice of positivly charged ions, cations, sorounded by free/ delocalised elctrons

electrostatic force of attraction between lattice of metal cations and sea off delocalised electrons

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2
Q

characteristics of metalic bonding

A

high melting and boiling point, because lots of energy needed to break strong electrostaic force of attraction

malleble and ductile, beaten into sheets, pulled in wires.- layers can slide over, can change shape but not break because of electrostatic force of attraction bewteen cations and electrons not broken

hard/ strong= difficult to compreess, and high tensi force

lusturous- electrons form barrier which reflects light

sonorous- reflects sounds/ condicts

conducts heat and energy- 1, electrons vibrate collide with cations and conduct heat// 2, electrons can carry charge

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3
Q

alloys// characteristics

A

combination/ mixture of 2 or more metals

  1. harder then pure metal
  2. less malleble,
  3. poorer conductors then pure metals
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4
Q

ionic compunds

A

made of cations which loses an electron and transfer it to an anion which gains the electron.

forms a giant ionic lattice- strong electrostatic force of attraction occurs between the oppositiely charged ions.

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5
Q

ionic compound characteristics

A 
brittle
high melting and boiling point
soluble in molten and water solutions
cant conduct electricity in solid 
conduct electricity in solutions
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6
Q 
polyatomic ions 
aretate 
nitrate 
hydroxide 
permanganate 
cyanide 
sulfate
carbonate 
chromade 
dichromade 
ammoniam
A 
CH3OO - 
OH- 
MnO4 -
CN-
SO4 -2 
CO3 2-
Cr04 2-
PO4 3-
NH4 1+
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7
Q

covalent bonding

A

is a bond between shared pairs of electrons,.

electrostatic force of attraction between the nuclei of 2 atoms and 1 or more shared pairs of electrons

some can expand ast 8 electrons- sulfur hexaflurine

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8
Q

dative covalent bonds

A

covalent bond in which shared electrons contributed by 1 atom

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9
Q

electron repulsion theory

A

shape of a molecule is determind by the number of electron pairs sorounding the centeral atom

affects melting and boiling point/ hardness and solubility

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10
Q

linear shape

A

2 bonding pairs, at 180 degrees

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11
Q

trigonal planar

A

3 bonding pairs, 120 degree angles

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12
Q

tetrahedral

A

4 bonding pairs at 109.5 degrees

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13
Q

trigonal pyramid

A

1 lone pair, angles are approx 109.5

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14
Q

v shaped/ bent

A

2 lone pairs

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15
Q

linear shape/ diatomic

A

3 lone pairs

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16
Q

lone pairs

A

more repulsive because greater electron denisty and will repel more bonded pairs, pushing a pair down 2.5 degrees

17
Q

covalent molecules characteristics

A

low melting and boiling point

do not conduct electrictiy

18
Q

giant covalent networks

A

high melting and boiling point
x conduct elec
very hard
insoluble

19
Q

alotropes

A

an alternative structured form of an element

20
Q

diamond

A

giant covalent network

carbon bonded to 4 others covalently in tetrahedral shape
hard insulator

high melting because requires large amount of energy to break strong c bonds
x conduct electricity because no free moving charged particles

21
Q

silcion dioxide

A

2 silcons covalently bonded to an oxygen tetrahedral shape

22
Q

graphite

A

insoluble/ high melting bp
soft used as lube
conducts electrcitiy because 1 unbonded electron freely able to move

23
Q

dispersion

A

intermolecular forces,
occurs between all molecules due to constant movement of electrons

very weak

greater surface area- greater area for forces to act across- requires more energy to change state
greater amount of electrons greater temp dipole

24
Q

dipole dipole

A

intermolecular force
occurs when there is a differenc in electronegativivty leads to one with greater electroneg having greater pull on other side,

greater electroneg- means delta neg other side delta pos

when 2 dipoles attract- b/w polar molecules

25
Q

polar

A

uneven distribution of charge and electrons

NOT POLAR IF WHOLE OUTSIDE IS DELTA POS, TETRAHEDRAL SHAPE

26
Q

hydrogen bonding

A

when the hydrogen in bonded to NOF in a molecules expeirence a strong intemolecular force between a lone pair of eleectrons on a NOF

Chemistry Units 1/2 (9 decks)

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