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IB Chemistry SL > Chemical Bonding + Structure > Flashcards

Chemical Bonding + Structure Flashcards

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1
Q

what is an ionic bond

A
  • electrostatic attraction between oppositivley charged ions
  • transfer of electrons
  • polarity difference greater than 1.7
  • usually metal + non metal (cations and anions)
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2
Q

what is a covalent bond

A
  • electrostatic attraction between a pair of electrons and a positively charged nuclei
  • sharing of electrons
  • usually nonmetal+ nonmetal
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3
Q

what is metallic bond

A
  • negatively charged metal ions are attracted to delocalized electrons
  • metal + metal
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4
Q

what are ionic compounds

A

are formed when electrons are transferred from one atom to another to form ions with complete outer shells of electrons
- consist of ions held tightly together in attic structures by ionic bonds

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5
Q

what are polyatomic ions

A

ions containing more than one elements

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6
Q

CATIONS

A

metals LOSE electrons to form positive ions

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7
Q

ANIONS

A

non-metals gain electrons to form negative ions

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8
Q

how can charge be predicted

A

accorrding to position on periodic table

- transition metals can form more than one charge

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9
Q

properties of ionic compounds

A
  • solids
  • lattice structure
  • high melting point + boiling point
  • low volatility
  • do NOT conduct electricity in solid state
  • soluble in water
  • neutrally charged due to balance of positive and negative ions
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10
Q

what is the goal of a covalent bond

A

octet rule/stability: to achieve a full shell of valance electrons

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11
Q

WHAT IS A MOLECULE

A

a group of atoms held together by covalent bonds

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12
Q

what happens as more bonds are added

A

bond length decreases and bond strength increases

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13
Q

what is electronegativity

A

the tendency of an atom in a molecule to attracted a shared pair of electrons towards itself

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14
Q

what is polarity

A

polar bonds form when two atoms bonded together have different electronegativity values (UNEQUAL SHARING)

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15
Q

what is VSEPR

A

VALANCE SHELL ELECTRON PAIR REPULSION: the total # of electron domains determine the geometrical arrangement by maximum repulsion

  • ELECTRONS ARRANGE THEMSELVES AROUND A CENTRAL ATOM SO THA THEY ARE AS FAR APART AS POSSIBLE
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16
Q

Linear

A

electron domains: 2 (2 atoms bonded to central atom)

angle: 180

17
Q

Bent/V-shaped

A

electron domain: 3 (2 atoms bonded to central atom with one or two un paired electrons)

angle: 105

18
Q

Trigonal Planear

A

electron domain: 3 ( 3 atoms bonded to central atom)

angle: 120

19
Q

trigonal pyramidal

A

electron domain: 4 (3 atoms and an unbonded pair bonded to central atom)

angle: 107 or less than 109.5

20
Q

tetrahedral

A

electron domain: 4 (4 atoms bonded to central atom)

angle: 109.5

21
Q

having polar bonds does not equal a polar molecule

A

symmetrically also is taken into account

22
Q

what are intermolecular forces

A

the physical properties of molecular substances that result from different type of forces between their molecules

23
Q

types of intermolecular forces

A
  • van der waal forces
  • london forces (dispersion forces)
  • dipole-dipole forces
  • hydrogen bonding
24
Q

what are london dispersion forces

A
  • temporary dipoles due to fluctuating electrical field
  • electrons can be unevenly spread which lead stop temporary dipoles

trend: increase with increasing molecular mass

25
Q

factors that affect the magnitude of london forces

A
  • number of electrons
  • size and volume of electron cloud
  • shapes of molecules
26
Q

what are dipole-dipole forces

A
  • when dipoles attract (usually in polar molecules)

- weaker than covalent bonds

27
Q

what are hydrogen bonds

A
  • a strong type of dipole-dipole
  • when hydrogen bonds to a small, highly electronegative element
    F, N
28
Q

strength of the forces

A

van der waal

29
Q

melting + boiling point

A

are an indication of the strength of the intermolecular forces

30
Q

m+ b points of covalent bonding

A

STRONG

31
Q

m+ b point of ionic and metallic bonding

A

strong due to ionic attraction

32
Q

the weaker the attractive forces….

A

the more volatile (boiling point) the substance

33
Q

m/b point of intermolecular forces

A

h bonding > dipole-dipole> london forces

34
Q

what is conductivity

A

substance must posses electrons.ions free to move

35
Q

covalent bond conductivity

A

WEAK CONDUCTORS UNLESS ABLE TO IONIZE SOLUTION

36
Q

Solubility

A

“Like dissolves like”

polar substances are more soluble in water and less soluble in non-polar substances

IB Chemistry SL (7 decks)

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