bonding Flashcards

1
Q

what do bonds between atoms always involve

A

outer electrons

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2
Q

why are noble gases very unreactive

A

because their outer main levels are full so have no need to react

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3
Q

why do atoms bond together

A

they will share or transfer electrons to gain a more stable electron configuration like noble gases - be jelly!!!

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4
Q

what is ionic bonding between

A

between oppositely charged ions and they will transfer their electrons from metal to non metal shells to obtain the full main outer level

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5
Q

what will happen as a result of ionic bonding

A

the metal will become positively charged - looses an electron - cation

the non- metal will become negatively charged gains the electrons from the metal - an anion

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6
Q

what force joins ionic compounds together

A

electrostatic forces of attraction

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7
Q

what are some properties of ionic compounds

A
  • solids at room temp
  • brittle - this is because of the oppositely charged ions and a blow in the wrong direction could cause the ions to come into contact that have like charged
  • only conduct electricity when molten
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8
Q

why are ionic compounds solids at room temp

A

because of their macromolecular ionic lattice and the large electrostatic forces of attraction between the ions the amount of energy required to overcome these forces is so large so it will remain solid until large amount of energy is applied.

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9
Q

why can ionic compounds only conduct elec when molten

A

because when in their giant ionic lattice delocalised electrons are not free to move throughout the structure but when it becomes molten or aqueous the soltion provide a place for delocalised electrons to carry charge

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10
Q

what is a covalent bond

A

bonding between a shared pair of electrons in a non-metal

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11
Q

what is the force of attraction between the nucleus and the electrons called

A

electrostatic

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12
Q

what are properties composed of molecules

A

low bpt and mpt - this is because strong covalent bonds are only between the atoms WITHIN MOLECULES
- poor conductors of elec - because the molecules are overall neutral and there are no delocalised electrons to carry charge throughout no structure!

  • even if the molecules dissolve into an aqueous solution they will not comduct elec because the molecules will remain molecules
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13
Q

what is co-oordinate bonding

A

in most covalent bonding the shared pair of electrons will come from both atoms but in coordinate bonding it comes only from one atom

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14
Q

what is a lone pair in coordinate bonding

A

the atom that is donating a pair of electrons to an electron deficient atom will donate a LONE PAIR to complete the outer shell

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15
Q

will coordinate bonding affect the shape of an molecule

A

no, though the electrons are only gifted from one atom the shape will be unaffected

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16
Q

where will the arrow in coordinate bonding go from to?

A

from the lone pair to where it is going

17
Q

what is the only difference between coordinately bonded covalent bonds and covalent bonds

A

coordinate bonds are charged whereas the covalent bonds are not

18
Q

what is metallic bonding

A

a lattice of positive ions existing in a sea of outer electrons - these outer electrons are delocalised which means they are not tied to a particular atom and so area ble to carry charge easily throughout the structure

19
Q

what does the number of delocalised electrons in the sea of electrons depend upon

A

how many electrons have been lost by each metal atom

20
Q

what are properties of metals

A
  • good conductors of heat and electricity
  • malleable - can be beaten into shape
    ductile - can be pulled into thin wires
    metals are ductile nad malleable because after small distortion ecah metal ion is still in the same environment so the new shape will be retained

high mpt - because they have a giant structures and there is a strong attraction between the metal ions and the delocalised sea of electrons which will make the atoms difficult to separate

21
Q

define electronegativity

A

the power of an atom to attract the electron density towards itself within a covalent bond

22
Q

define polarity

A

the equal sharing of electrons that are bonded together covalently

23
Q

which factors will affect electronegativity

A
  • nuclear charge
  • the distance between the nucleus and the outer shell
    shielding of the nuclear charge by electrons in the inner shell.
24
Q

what is the trend in electroneg

A

increases across a period and up a group so the most electronegative element is fluorine 4.0 woohoo

25
Q

what can a difference in electronegativity cause

A

a dipole

26
Q

what is a dipole - may you ask

A

a difference in charge between two atoms caused by a shift in electron density

27
Q

are electrons static

A

noo - electrons are constantly moving in their electron clou thi is how you achieve van der waals and induced dipoles

28
Q

what does a molecule having a permanent or induced dipole depend upon

A

its shape and polarity

29
Q

what is a symmetric molecule???

A

all bonds are identical and no lone pairs. will not be polar even if individual bonds are polar. the individual dipoles can cancel out… the negatives will all cancel and positives can cancel it is not nessacerialy in equilibrium Cl4 see google for more you poor sod

30
Q

who came up with the electroneg scale

A

pauling