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Chemistry > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

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1
Q

What is a compound?

A

2 or more different elements chemically combined

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2
Q

How are atoms held together?

A

chemical bonds

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3
Q

describe noble gases

A

contain 8 elements on outer shell and are generally unreactive

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4
Q

what are the uses of helium

A

airships and balloons

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5
Q

uses of argon

A

Used in lightbulbs (normal light bulbs) to stop imploding

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6
Q

what is the octet rule

A

in forming compounds, atoms tend to achieve the electron configuration of a noble gas(8 electrons)

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7
Q

what are the limitations of the octet rule

A

hydrogen, lithium, transition elements

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8
Q

what is a valency

A

it is the no. of bonds an atom makes when it reacts

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9
Q

what is a transition metal

A

it is one that forms at least one ion with a particularly filled sublevel

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10
Q

facts about transition metals

A

they have variable valancy

form coloured compounds

used as catalysts

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11
Q

name 2 types of bonding

A

ionic,convalant

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12
Q

what is an ion

A

a charged atom/groups of atoms

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13
Q

what is the charge of a cation

A

positive

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14
Q

what is the charge of a anion

A

negative

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15
Q

define ionic bonds

A

the attraction between oppositely charged ions in a compound

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16
Q

why do ionic substances form substances

A

positive ions attract negative ions in all direcions

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17
Q

what are the characteristics of ionic substances

A
  • strong forces between ions means its very hard to –break up the lattice structure
  • can conduct electricity when solid
  • high melting/boiling points
  • most dissolve in water
  • solid at room temp
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18
Q

examples of everyday ionic substances

A

table salt-Sodium Chloride (NaCl)

fluoridation in water-SodiumFlouride(NaF)

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19
Q

When is a covalent bond formed?

A

when electrons are shared between atoms

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20
Q

what are bonding pairs

A

shared electron pairs that form covalent bonds

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21
Q

What are lone pairs?

A

electron pairs not involved in bonding

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22
Q

How is a sigma bond formed?

A

formed by the head overlap of two orbitals (can be s/p orbitals)

23
Q

how is a pi bond formed

A

formed by sideways overlap of p-orbitals

24
Q

which is stronger sigma vs pi bonds

A

sigma bonds are stronger due to the fact that there is more overlap between orbitals

25
Q

what are the characteristics of ionic bonds

A
  • transfer of electrons
  • ions formed
  • high melting/boiling point
  • usually solid at room temp
  • conducts electricity when molten
26
Q

what are the characteristics of covalent bonds

A
  • sharing electrons
  • covalent bonds formed
  • low melting/boiling points
  • liquid/gaseous at room temp
  • deosnt conduct electricity
27
Q

what is In a single bond

A

one sigma

28
Q

what is in a double bond

A

one sigma, one pi

29
Q

what is in a triple bond

A

one sigma, two pi

30
Q

How are molecules formed?

A

Covalent bonds between two or more atoms.

31
Q

How is the shape of a molecule determined?

A

the arrangement of atoms

32
Q

what theory is used to figure up the arrangement of molecules

A

VSEPR- valance shell electron pair repulsion theory

33
Q

describe why the shape of lone and bonding pairs are disstorted(explain the basis for electron pair repulsion pair theory(i think))oooop

A
  1. lone pair electrons are closer to the nucleus
  2. due to this it they are closer together
  3. collective nuclear charge pushes the bonding pairs further apart

decreasing the bond angle+distorts the shape

electrons in bonding pairs repel each other and want to be as far away as possible

34
Q

no. of bonding pairs around the central atom and angle of a linear molecule

A

2 atoms and 180 degrees

35
Q

no. of bonding pairs around the central atom and angle of a trigonal planar atom

A

3 atoms and 120 degrees

36
Q

no. of bonding pairs around the central atom and angle of a tetrehedral atom

A

4 atoms and 109.5 degrees

37
Q

what are lone pairs

A

Paired electrons that are not shared

38
Q

what is a molecule, no of bonding pairs,no of lone pairs, bod angle of a pyramidal molecule

A

NH3, 3, 1 ,107 degrees

39
Q

what is a molecule, no of bonding pairs,no of lone pairs, bod angle of a V-Shaped molecule

A

H20, 2 , 2, 104.5 Degrees

40
Q

What are non-polar covalent bonds?

A

equal sharing of electrons

41
Q

What are polar covalent bonds?

A

unequal sharing of electrons

42
Q

Define Elecronegativity

A

its the relative attraction an atom has for a shared pair of electrons in a single covelent bond

43
Q

what are the trends in the periodic table in terms of electromagnetically

A

Increase across the table=increase in nuclear charges/decreased atomic radius

Decrease down the table=screening/increase atomic radius

44
Q

how do you predict the type of bond an atom has

A

check the electronegativity of the atoms involved

calculate the difference in electronegativity

45
Q

what is the bond type of atoms with the electronegativity of non-polar covelant bonds

A

0-0.4 ex-H2,O2

46
Q

what is the bond type of atoms with the electronegativity of polar covelant bonds

A

0.41-1.7 example-H20

47
Q

what is the bond type of atoms with the electronegativity of Ionic bonds

A

greater than 1.7 example-NaCl

48
Q

a molecule that has polar bonds can be non-polar overall if its one of the following shapes

A

linear,trigonal planar, tetrahedral

49
Q

What is intramolecular force?

A

force within a molecule

50
Q

What is intermolecular force?

A

force between molecules

51
Q

what are the three types of molecular bonding

A

Van Der Waal

Dipole-Dipole

Hydrogen bonding

52
Q

What are Van der Waals forces?

A

weak forces of attraction between temporary dipoles

53
Q

What are dipole-dipole forces?

A

forces of attraction between negative polar of one molecule and the positive pole of another

54
Q

What are hydrogen bonds?

A

occurs in molecules where a hydrogen atom is bonded to nitrogen,oxygen,fluorine. the hydrogen carries a positive charge and is attracted to the electronegative in another molecule

Chemistry (12 decks)

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