atomic structure

Question 1

what is it and where does metallic bonding occur?

Answer 1

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

Question 2

metallic bonding structure

Answer 2

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

Question 3

metallic bonding properties

Answer 3

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)

Question 4

identifying bonding and structure

Answer 4

-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

Question 5

how do ionic substances have specific properties?

Answer 5

by the type of particles and forces present

Question 6

when does ionic bonding occur

Answer 6

between oppositely charged ions

Question 7

what is ionic bonding

Answer 7

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

Question 8

bonding

Answer 8

describes the way that particles “join” together

Question 9

structure

Answer 9

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

Question 10

covalent bonding

Answer 10

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

Question 11

what is an atom

Answer 11

smallest unit of matter that retains its properties

Question 12

what are subatomic particles

Answer 12

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

Question 13

particles and their relative mass and charge

Answer 13

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

Question 14

atomic number

Answer 14

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

Question 15

atoms are…

Answer 15

neutral, therefore number of protons = number of electrons

Question 16

mass number

Answer 16

number of protons + no of neutrons

Question 17

neutrons

Answer 17

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

Question 18

isotopes

Answer 18

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

Question 19

element

Answer 19

a substance made of atoms with the same number of protons

Question 20

pure

Answer 20

only an element present (same protons)

Question 21

isotopically pure

Answer 21

only one isotope (same protons, same neutrons)

Question 22

ion

Answer 22

charged atom or molecule
cation= positive
anion= negative

Question 23

when do particles become charged

Answer 23

when protons =/ electrons

Question 24

why can electrons be easily gained or lost

Answer 24

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

Question 25

ionic bond

Answer 25

electrostatic force of attraction between oppositely charged ions

Question 26

what is a lattice

Answer 26

a 3D repeating pattern

Question 27

structure of ionic bonding

Answer 27

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

Question 28

mpt/bpt of ionic bonding

Answer 28

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.

Question 29

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

Answer 29

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

Question 30

conductivity in ionic bonding

Answer 30

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.

Question 31

solubility in ionic bonding

Answer 31

dissolves in water

Question 32

maluability in ionic bonding

Answer 32

brittle, movement of ions in the lattice causes to repel

Question 33

why does covalent bonding share an electron

Answer 33

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

Question 34

covalent bond

Answer 34

electrostatic attraction of 2 nuclei for a shared pair of electrons

Question 35

what are the forces in covalent discrete

Answer 35

-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)

Question 36

properties for covalent discrete

Answer 36

-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.

Question 37

what are the 3 substances that have lattice covalent

Answer 37

SiO2: sand C: diamond, or graphite

Question 38

description of covalent lattice

Answer 38

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

Question 39

properties of covalent lattice

Answer 39

-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.

Question 40

what is diamond and graphite

Answer 40

both are different allotropes of carbon

Question 41

allotrope

Answer 41

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

Question 42

diamond properties

Answer 42

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

Question 43

graphite properties

Answer 43

-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.

Question 44

graphite and diamond structure

Answer 44

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

Question 45

protons

Answer 45

relative mass of 1 relative charge of 1

Question 46

electrons

Answer 46

relative mass of 1/2000 relative charge of -1

Question 47

calculating average mass of isotope (Ar)

Answer 47

abundance x mass the same ________________ + 100

Question 48

particles becomes charged when...

Answer 48

the number of protons =/ no. of electrons

Question 49

covalent structures have 2 types of bonding

Answer 49

strong covalent bonds in the molecule weak IMFs holding molecules together

Question 50

atomis mass

Answer 50

combined mass of protons and neutrons

Question 51

the more neutrons in isotopes

Answer 51

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