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atomic structure Flashcards

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1
Q

what is it and where does metallic bonding occur?

A

-in metallic elements and alloys
-no transferring or sharing of electrons
-atoms have weak attraction
-everything is attracted

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2
Q

metallic bonding structure

A

-can only form lattices (positive ions surrounded by delocalized electrons)
-atoms have weak attraction so they from delocalized electrons

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3
Q

metallic bonding properties

A

high mpt/bpt: strong electrostatic forces(more delocalized e-s the higer the mpt/bpt)
malleable, cations can move around without breaking the electrostatic forces
can conduct because delocalized e-s can move around(not as a gas)
insoluble in all solvents (can react)

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4
Q

identifying bonding and structure

A

-conductivity as a solid:
yes, metallic or graphite
no, ionic, covalent
-solubility in water:
yes, ionic(exceptions)
no, covalent(exceptions), metallic
-solubility in oils:
yes, covalent(discrete)(exceptions)
no, ionic, covalent (lattice)
-MPT:
yes, covalent discrete
no, ionic, covalent lattice, metallic
-conductivity liquid:
yes, ionic, metallic
no, covalent
-conductivity aquose:
yes, ionic
no, covalent, metallic, ionics that are insoluble

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5
Q

how do ionic substances have specific properties?

A

by the type of particles and forces present

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6
Q

when does ionic bonding occur

A

between oppositely charged ions

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7
Q

what is ionic bonding

A

when a compound contains at least one metal and one non-metal

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8
Q

bonding

A

describes the way that particles “join” together

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9
Q

structure

A

describes the 3D arrangement of particles as a result if bonding

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10
Q

covalent bonding

A

occurs between atoms of 2 non-metals.
the non-metals can be the same (element) or they can be different (compound)
the atoms share a electron

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11
Q

what is an atom

A

smallest unit of matter that retains its properties

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12
Q

what are subatomic particles

A

the 3 fundamental particles that constitute atoms:
proton, neutron, electron

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13
Q

particles and their relative mass and charge

A

proton: 1, +1
neutron: 1,0
electron: 1/1836, -1

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14
Q

atomic number

A

number of protons, definition of an element, the periodic table is listed in order of number of protons.

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15
Q

atoms are…

A

neutral, therefore number of protons = number of electrons

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16
Q

mass number

A

number of protons + no of neutrons

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17
Q

neutrons

A

mass number - atomic number
relative mass of 1
relative charge of 0

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18
Q

isotopes

A

-atoms of the same element with different numbers of neutrons
-they have identical chemical properties, they have similar but different physical properties

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19
Q

element

A

a substance made of atoms with the same number of protons

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20
Q

pure

A

only an element present (same protons)

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21
Q

isotopically pure

A

only one isotope (same protons, same neutrons)

22
Q

ion

A

charged atom or molecule
cation= positive
anion= negative

23
Q

when do particles become charged

A

when protons =/ electrons

24
Q

why can electrons be easily gained or lost

A

-the electrons are located on the outside of the atom(less energy required to remove)
-the electrons are much smaller than the protons

25
Q

ionic bond

A

electrostatic force of attraction between oppositely charged ions

26
Q

what is a lattice

A

a 3D repeating pattern

27
Q

structure of ionic bonding

A

lattice of alternating cations and anions that are held together with electrostatic forces

28
Q

mpt/bpt of ionic bonding

A

high melting point becuase of the electrostatic forces that are very strong and each ion has multiple attractive forces, therefore lots of energy is needed to weaken the forces.

29
Q

what does the strength of each force depend on in ionic bonding

A

magnitude of charge and the radius of each ion (the charge is more dispersed of bigger ions)

30
Q

conductivity in ionic bonding

A

charged particles are present (ions) but cannot conduct as a solid because they can’t move. as a liquid of dissolved they can move so they can conduct charge.

31
Q

solubility in ionic bonding

A

dissolves in water

32
Q

maluability in ionic bonding

A

brittle, movement of ions in the lattice causes to repel

33
Q

why does covalent bonding share an electron

A

because both atoms attract the shared electron equally and therefore the atoms join (molecule)

34
Q

covalent bond

A

electrostatic attraction of 2 nuclei for a shared pair of electrons

35
Q

what are the forces in covalent discrete

A

-strong covalent bonds that hold the molecule together. these only change during reactions
-weak IMFs holding groups of molecules together. these are affected by physical processes (melting dissolving)

36
Q

properties for covalent discrete

A

-low mpt/bpt; the weak IMFs require little energy to weaken. the mpt depends on the size of the molecules. (bigger more IMFs=higher mpt)
-do not conduct as they don’t have any charged particles
-soluble in oil like substances and low solubility in water. when they dissolve the molecules separate from each other breaking the IMFs.

37
Q

what are the 3 substances that have lattice covalent

A

SiO2: sand
C: diamond, or graphite

38
Q

description of covalent lattice

A

lattice of atoms held together with strong covalent bonds( no weak IMFs)

39
Q

properties of covalent lattice

A

-very high mpt because strong covalent bonds needing lots of energy to break
-does not conduct because no charged particles are present
-insoluble in all solvents
-brittle because the atoms can only move if the covalent bonds break, the bond cannot reform in the new position.

40
Q

what is diamond and graphite

A

both are different allotropes of carbon

41
Q

allotrope

A

different structural arrangements of the same element. same chemical properties but different physical properties.

42
Q

diamond properties

A

high mpt (covalent lattice)
doesn’t conduct
insoluble in all solvents
brittle

43
Q

graphite properties

A

-high mpt (same as diamond)
-conduct electricity as a solid because of delocalized electrons
-insoluble
-lubricant: layers of atoms can slide over each other without disrupting the rest of the lattice.

44
Q

graphite and diamond structure

A

graphite: lattice of atoms arranged in alternating layers w/ delocalized electrons (covalent lattice)
diamond: triangle based pyramid (covalent lattice)

45
Q

protons

A

relative mass of 1
relative charge of 1

46
Q

electrons

A

relative mass of 1/2000
relative charge of -1

47
Q

calculating average mass of isotope (Ar)

A

abundance x mass the same
________________ +
100

48
Q

particles becomes charged when…

A

the number of protons =/ no. of electrons

49
Q

covalent structures have 2 types of bonding

A

strong covalent bonds in the molecule
weak IMFs holding molecules together

50
Q

atomis mass

A

combined mass of protons and neutrons

51
Q

the more neutrons in isotopes

A

the greater mass = greater density
higher mpt –> can be seperated by fractional distallation

chemistry (10 decks)

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