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Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

*Orbital

A

A region around the nucleus that can hold up to two electrons, with opposite spins

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2
Q

*ionic bonding

A

The electrostatic attraction between oppositely charged ions.

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3
Q
  • covalent bonding
A

Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

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4
Q

*polar molecule

A

has polar bonds with dipoles that do not cancel due to their direction

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5
Q

*electronegativity

A

the ability of an atom to attract the bonding electrons in a covalent bond

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6
Q

Dipole

A

: partial charged atoms in a covalent bond due to different electronegativity

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7
Q

allotropes

A

different forms of the same element in the same state, e.g graphite and diamond

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8
Q

dative covalent bond

A

When both electrons come from one atom in a covalent bond.

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9
Q

when and why can ionic compounds conduct electricity

A

Ionic compounds don’t conduct as solid due to no mobile ions, they can conduct when molten/ in solution as ions are mobile.

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10
Q

can covalent compounds conduct electricity? why?

A

Covalent compounds can’t conduct as solids or liquids/solutions as they have no ions or mobile electrons.

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11
Q

can metals conduct electricity

A

Metals can conduct when solid or molten as they have delocalised electrons.

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12
Q

When explaining shapes of molecules or bond angles state:

A

o Number of bond pairs and lone pairs of electrons
o Electron pairs repel so spread out
o Lone pairs repel more than bonded pairs

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13
Q

what is an induced dipole- dipole

A

caused by movement of electrons causing a temporary dipole which induces a dipole in a neighbouring molecule. The more electrons a molecule has the larger the force, e.g. I2 has lots of electrons so induced dipole forces are strong enough that it’s a solid.

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14
Q

what is a permanent dipole

A

a difference in electronegativity causes a permanent dipole so molecules are attracted to each other.

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15
Q

what is hydrogen bonding

A

occurs between molecules that have N, O or F with a lone pair and H attached. Strong compared to other IM bonds

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16
Q

what are the rules of orbitals

A

the two electrons have opposite spins

the orbitals in he same sub shell fill up singly before pairing up

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17
Q

shape of s orbital

A

spherical

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18
Q

shape of p orbital

A

3d - dumbell shape

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19
Q

how many orbitals and electrons are in the s sub-shell

A

1 orbital

2 electrons

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20
Q

how many orbitals and electrons are in the p sub-shell

A

3 orbitals

6 electrons

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21
Q

how many orbitals and electrons are in the d sub-shell

A

5 orbitals

10 electrons

22
Q

how many orbitals and electrons are in the f sub-shell

A

7 orbitals

14 electrons

23
Q

what sub-shells are in the first shell (and electrons)

A

1s - 2 electrons

24
Q

what sub-shells are in the second shell (and electrons)

A

2s 2p - 8 electrons

25
Q

what sub-shells are in the third shell (and electrons)

A

3s 3p 3d - 18 electrons

26
Q

what sub-shells are in the fourth shell (and electrons)

A

4s 4p 4d 4f - 32 electrons

27
Q

what is a cation

A

metal ion

positive

28
Q

what is an anion

A

non-metal ion

negative

29
Q

what is a giant ionic lattice

A

giant regular structure with electrostatic attraction in all directions

30
Q

properties of ionic compounds

A
  • high melting and boiling point (strong bonds)
  • electrical conductor in liquids and solution
  • soluble in water (ions are attracted to the polar water molecules)
31
Q

what is average bond enthalpy

A

measures the energy required to break a covalent bond

32
Q

2 bonded pairs, 180 degrees

A

linear shape

33
Q

linear shape

A

2 bonded pairs, 180 degrees

34
Q

3 bonded pairs, 120 degrees

A

trigonal planar

35
Q

trigonal planar

A

3 bonded pairs, 120 degrees

36
Q

tetrahedral

A

4 bonded pairs, 109.5 degrees

37
Q

4 bonded pairs, 109.5 degrees

A

tetrahedral

38
Q

3 bonded pairs, 107 degrees

A

trigonal pyramidal

39
Q

trigonal pyramidal

A

3 bonded pairs, 107 degrees

40
Q

bent/ non-linear

A

2 bonded pairs, 2 lone pairs, 104.5 degrees

41
Q

2 bonded pairs, 2 lone pairs, 104.5 degrees

A

bent/ non-linear

42
Q

trigonal bi pyramidal

A

5 bonded pairs, 120 degrees, 90 degrees

43
Q

5 bonded pairs, 120 degrees, 90 degrees

A

trigonal bi pyramidal

44
Q

octrahedral

A

6 bonded pairs, 90 degrees

45
Q

6 bonded pairs , 90 degrees

A

octrahedral

46
Q

what is a polar bond

A

a bond where the electron are unevenly distributed due to a difference in electronegativity

47
Q

why is ice less dense than water

A

long hydrogen bonds break making water denser

48
Q

why does water have a relatively high melting point

A

stronger inter molecular forces (hydrogen)

49
Q

when does hydrogen bonding happen

A

hydrogen with fluorine, nitrogen, oxygen

50
Q

why do simple covalent compounds have low melting points

A

inter molecular forces are weaker than intramolecular forces

51
Q

why are polar molecules soluble in water (s.c.)

A

dissolves polar molecules or forms hydrogen bonds

52
Q

what do simple covalent not conduct electricity

A

overall uncharged

Chemistry (12 decks)

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