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Grade 12 Chemistry > Atomic Structures Part 2 > Flashcards

Atomic Structures Part 2 Flashcards

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1
Q

what is an ionic bond. How does it work?

A

an actual transfer of electrons from the metal and the non-metal. The transfer creates two opposite charges that are attracted to eachother holding them together

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2
Q

what are the two components of an ionic bond

A

an element with low ionization energy (metal) and an element with a high ionization energy (non metal)

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3
Q

describe an ionic solid at room temperature

A

they are solid because of the attraction between the ions is very strong

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4
Q

how are atoms arranged in an ionic solid?

A

in a highly ordered crystal lattice structure, maximizing attractive forces and minimizes repulsive forces

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5
Q

how to ionic compounds behave in water

A

are slightly soluble and will conduct electricity as ions are free to move to oppositely charged electrodes

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6
Q

what is a covalent bond

A

when electrons are shared between nucleuses to achieve a full outer energy level

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7
Q

what type of atoms are present in a covalent bond?

A

2 atoms with high ionization energies

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8
Q

in a covalent bond when are electrons shared equally?

A

when the electronegativity different between the atoms is less than 0.4

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9
Q

in a covalent bond when is it a polar bond?

A

the electronegativity difference between the two atoms is between 0.4 and 1.7 which leads to an unequal sharing of electrons

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10
Q

when will a MOLECULE be polar?

A

if it is assymmetrical and contains polar covalent bonds

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11
Q

what is a coordinate covalent bond

A

when both electrons being shared come from the same atom

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12
Q

describe non-polar covalent solids by themself

A

have low melting and boiling points and are often gases at room temperature due to the low intermolecular forces that exist in these molecules (LDF only)

if they are solid at room temperature usually soft and waxy

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13
Q

describe non-polar covalent solids in water

A

soluble in non-polar solvents like etheres, but won’t conduct electricity as they lack charged components

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14
Q

what are some properties of polar covalent molecules

A

tend to have higher melting and boiling points and are more likely to be liquids or solids at room temp

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15
Q

describe polar covalent molecules in water

A

will dissolve in polar solvents and will not conudct electrivity as very few particles to ionize

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16
Q

what is a metallic bond?

A

when both atoms have low ionization energies and low electronegativities and will lose electrons easily - like 2 metals

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17
Q

describe the electrons in a metallic bond

A

positive metal ions are arranged with valence electrons delocalized around them, thus they are mobile and move throughout the metal structure

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18
Q

what are the properties of metallic compounds

A
  • malleable and ductile
  • good conudctors of heat and electricity
  • shiny
  • solid at room temp
  • have a photoelectric effect
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19
Q

why are metallic ompounds malleable and ductile?

A

atoms are restrictied to one position by a fixed bons and the ions can roll past each other

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20
Q

why are metallic compounds good conductors of heat and electricity

A

because electrons are mobile and can’t transmit energy rapidly

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21
Q

why are metallic compounds shiny?

A

because when light strikes a metal the valence electrons absorb energy and oscillate at the same frequency as the incidient light and then emit light as a reflection of the original light

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22
Q

why are metallic compounds solid at room temperature?

A

due to the strong bonds

23
Q

what is the photoelectric effect?

A

electron emission caused by heat or light occurs when the frequency of light strikin a metal is sufficient to overcome to attractive forces and an electron escapes the metal decreasing the energy of the photon

24
Q

what is a network solid?

A

a macromolecule - a gient structure of covalently bonded atoms in one, two or three dimensional arrays

25
Q

what are allotropes?

A

elements that exist in different physical forms with different physical properties but the same chemical properties

26
Q

what is a 3-dimensional network solid?

A

network solid consists of covalently bonded atoms which form regular 3-D arrays or crystals

27
Q

what are some properties of 3-dimensional network solids

A
  • very strong bonds s
  • high melting and boiling points
  • solid and room temperature, be extremely hard
  • not soluble in any solvent
  • do not conduct electricity
28
Q

what are some examples of 3-dimensional network solids?

A

diamond, quartz, and silicon carbide

29
Q

what is a 2-dimensional network solids

A

network of covalent bonds that form 2-D arrays or sheets
the layers are held together by van del Waals forces

30
Q

describe the properties of 2-dimensional network solids

A
  • high melting and boiling points
  • soft and the layers will slides over each other allowing them to be used as a lubraicant
31
Q

what is an example of 2-dimensional network solids

A

graphite

32
Q

what is a 1-dimensional network solids

A

solids that form networks of a one dimension array or fibre - a long chain held together by covalent bonds - between adjacent chains attractive forces are very weak

33
Q

describe the properties of 1-dimensional network solids

A
  • very high melting and boiling points due to strong covalent bonds
  • solid and room temp
  • NOT soluble in water
34
Q

what is an example of a 1-dimensional network solid

A

asbestos

35
Q

describe quartz

A
  • 3-dimensional network
  • each silicon tetrahedrally bonded to four oxygen atoms
  • foreign metal ions in quartz produce semiprecious stone like emerald, amethyst and garnet
36
Q

describe mica

A
  • 2-dimensional sheets of silicate Si + O
  • mica flakes
37
Q

who came up with the valence bond model?

A

Linus Pauling

38
Q

What does the valence bond model say?

A

it exists to explain how atoms come together to form molecules

covalent bonds form when two orbitals overlap to produce a new combined orbital containing two electrons of opposite spin which results in a decrease in the energy of the atoms forming the bond, most likely to found between the two nuclei forming the bonds

39
Q

what must be true for atoms to bond according to the valence bond model?

A

the orbitals combining must start with an unpaired electron

40
Q

what was wrong with the valence bond theory?

A

cannot be used to explain the bonding in most covalent compounds and polyatomic ions and cannot be used to explain multiple bonds

41
Q

what points from the valence bond theory remained valid?

A
  1. simple molecules can bond according to the valence bond theory with regular orbitals
  2. a covalent bond results from the overlapping of 1 orbital from each atom in the bond.
42
Q

what does hybridization theory hypothesize?

A

the central atom makes new orbitals before bonding with the other atom, which are called hybrid orbitals

43
Q

how are hybrid orbitals formed?

A

by combining the atom’s atomic s, p and d orbitals

44
Q

what must be true for hybrid orbitals to be created?

A

the orbitals being combined must all come from the same energy level

and for each hybrid orbital needed you must use 1 atomi orbital

45
Q

the set of byhrib orbitals all have equal energy

A
46
Q

when are hybrid orbitals needed?

A
  1. sigma bonds
  2. lone pairs
  3. co-ordinate covalent bonds
47
Q

what is a sigma bond?

A

1 hybrid orbital with a electron

48
Q

what is a lone pair

A

1 hybrid orbital with 2 electrons

49
Q

describe a co-ordinate covalent bon in relation to hybrid orbitals

A

1 hybrid orbital with 2 electrons or an empty hybrid orbital

50
Q

what is a pi bond?

A

additional bond to make double/triple bonds

51
Q

describe a pi bond

A

do not hybrid orbitals - formed using regular atomic p orbitals with 1 electron

52
Q

what is a bonding orbital

A

lower energy and greate stability this is where there is a greater possibility to find the electrons between the nuclei of the atom

53
Q

what is an antibonding orbital

A

higher energy and lower stability, low possibility to find the electrons between the nuclei of the atom

54
Q
A

Grade 12 Chemistry (10 decks)

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