Chemistry Flashcards

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1
Q

name the mass and charge of each atomic particle

A

proton (mass=1 charge=+1) neutron (mass=1 charge=0) electron (mass=0 charge=-1)

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2
Q

define an isotope

A

Atoms of the same element and same atomic number with different numbers of neutrons and different mass number

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3
Q

define relative molecular mass

A

total mass of all the atoms in the ionic formula

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4
Q

how to work out moles

A

mass/Ar or Mr

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5
Q

what is concentration measured in

A

g/dm^3 or mol/dm^3

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6
Q

how to calculate the number of moles in a solution

A

concentration (mol.dm^-3) X volume (cm^3)

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7
Q

how to calculate the volume

A

volume (dm^3)=24 X moles

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8
Q

how do you measure atomic radius

A

measure the distance between two nuclei and divide by two

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9
Q

what happens to atomic radius across a period

A

decreases

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10
Q

what happens to atomic radius as you go down a group

A

increases

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11
Q

what is ionisation energy

A

electrons being removed from atoms and the energy it takes to remove them can be measured. Atoms become positive ions.

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12
Q

what does the ionisation energy of an element depend on

A

atomic radius nuclear charge (number of protons) number of electron shells

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13
Q

what is a molecular formular

A

refers specifically to a covalently bonded molecule and shows the number of atoms of each element in molecules of a particular compound

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14
Q

what is a empirical formula

A

refers to ionic or covalent compounds and is the simplest ratio of atoms of different elements in a compound

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15
Q

how do you work out the volume in an ideal gas equation

A

v= nRT/P

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16
Q

how do you work out the number of moles n of a gas in an ideal gas equation

A

n=PV/RT

17
Q

Structure of diamond

A
  • Tetrahedral structure
  • Each carbon is bonded to 4 other carbons
  • Carbons are covalently bonded
18
Q

properties of diamond

A
  • very hugh melting point (2000°C)
  • no charged oarticles, does not conduct electricty
  • dosen’t dissolve in any olvent
19
Q

structure of giant covalent:graphit

A
  • hexagonal arrangment of carbons
  • each carbon bonds to 3 other carbons
  • covalent bond
  • forms layer
20
Q

structure of graphene

A
  • single layer of graphite
  • giant covalent lattice, high melting and boiling point
  • dosen’t dissolve in any solvent
  • conduct electricty, delocalised electrons
  • transparent, extremely thin
21
Q

properties of graphite

A
  • high melting point
  • does not dissolve in any solvent
  • soft and sippery
  • conduct electricty
22
Q

structure of fullerenes

A
  • 60 carbon atoms joined together to form a ball
  • giant lattice, high melting and boling point, insoluble
  • conducts electricty
23
Q

properties of ilicion dioxide

A
  • lagre number of strong covalent bonds
  • high melting and boiling point
  • had crystaline structure
  • cannot conduct electricty
24
Q

Metal atoms …. outer ecltrons and become …..

A
  • loose
  • positive
25
Q

Free elctrons are called

A
26
Q

What are the properties of metallic bonding?

A
  • High melting points
  • Hard and strong
  • Solid at room temperature
  • Conduct elctricty and heat