1-Atomic Structure And The Periodic Table Flashcards
What is the relative mass and charge of a proton
Mass=1
Charge=+1
What is the relative mass and charge of a neutron
Relative mass=1
Charge=0
What is the charge and relative mass of an electron
Mass=1/2000 can be taken as 0
Charge= -1
What does the atomic number show
How many protons there are
What does the mass number show
The total number of protons and neutrons in the atom
What is an element
A substance that only contains the same atoms
What is an isotope
Different forms of the same element, which have the same number of protons but a different number of neutrons
What is a common example of isotopes
Carbon-12 and Carbon-13
What is the equation for calculating relative formula mass linking to isotopes
Relative formula mass(Ar) = sum of (isotope abundance x isotope mass number) / sum of abundance of all the isotope
How can equations be balanced
Putting numbers in front of the formulas where needed
What does chromatography separate
Dyes and inks
Why do u use a pencil line in chromatography
Because it is insoluble so it won’t affect the dyes
What is the end pattern in chromatography called
A chromatogram
What does filtration separate
An insoluble solid and a liquid
What are the two ways to separate a soluble salt from a solution
Evaporation and crystallisation
What is simple distillation used for
Separating a liquid from a liquid
What is fractional distillation used for
Separating out a mixture of liquids
What are the key pieces of equipment is used in fractional distillation
Fractionating column, condenser
What was John Dalton’s theory of atomic structure
Atoms were solid spheres that could not be separated
What was JJ Thomson’s model of the atom called
The plum pudding model
What was the plum pudding model
A ball of positive charge with electrons stuck in it
What was Rutherford’s experiment called
The alpha particle scattering experiment
What was the alpha particle scattering experiment
Alpha particles were fired at gold foil
What happened to the alpha particles in the scattering experiment
Most of them went straight through, some were deflected and some came straight back
What was concluded from the scattering experiment
The nuclear model was made which had a tiny positively charge nucleus in the centre with a cloud of electrons around it
What did Neils Bohr suggest about the structure of the atom
The electrons orbited the nucleus in shells at fixed distances
What did James Chadwick’s experiment prove the existence of
Neutrons
How many electrons can there be in the first 4 shells
2
8
8
2
How did Mendeleev order his period table
Mainly in order of atomic mass but did switch some so that the properties were similar
Why did Mendeleev leave gaps
So that elements with similar properties stayed in groups
What r the properties of metals
Strong, malleable, good conductors, High b.p and m.p
What r the properties of non-metals
Brittle, dull looking, don’t generally conduct, low b.p and m.p
What r the properties of transition metals
Very dense, strong and shiny. Good conductors
Can have more than one ion.
Often coloured.
Catalysts
What r the trends of group one metals as u go down the periods
Increasing reactivity
Lower melting and boiling points
Higher relative atomic mass
Why do group 1 elements get more reactive as u go down
Because the outer electron gets further away from the nucleus and the attraction decreases so it is more easily lost
What do group 1 metals react with water to produce
Hydrogen gas and metal hydroxides
What do group 1 metals produce when they react with chlorine
Chlorine gas and white metal chloride salts
What do group 1 metals produce when they react with oxygen
A metal oxide
What r the trends of group 7 elements as go down the periods
Less reactive
Higher melting and boiling points
Higher relative atomic mass
What are the acronyms for metals and non metals gaining and losing electrons
MALE
NAGE
Why don’t group 0 elements react
Because the have a full outer shell and are already stable
