Year 10 Mock Flashcards
What is an isotope
An isotope is an element with Sam’s number of protons but different numbers of neutrons
What’s the reaction of gas to water
Condensing
Liquid to gas
Evaporation
Solid to liquid
Melting
Liquid to solid
Freezing
Order of history of atoms individuals and what did they do
Dalton small ball , jj Thompson plumb pudding, Rutherford Geiger and marsdon gold foil experiment, Bohr electron shells.
Relative mass of proton neutron and electron
Proton 1 neutron 1 electron 0.0005
Relative charge of proton neutron and electron
Proton = 1 neutron = 0 electron = - 1
What’s a molecule
Two or more atoms
What’s the mass number
Bigger number
What’s the atomic number
Smaller number
What does mass number represent
Total number of protons and neutrons
What does atomic number represent
Number of protons
How to find number of protons
Atomic number
How to find number of neutrons
Mass number - atomic number
How to find out electrons
In normal uncharged atom electron is same as atomic number however charge affects number of electrons. E.g x- means that there’s an extra electron
What’s an isotope
Isotopes are different forms of same element with different number of proton but different numbers of electrons
Who created first periodic table
Dimitri Mendeleev in 1869
Why did dimitri include gaps
As he predicted there would be more elements
What does group number = in terms of electron’s on outer shell
Group number = number of electrons on outer shell
How to find number of shells on periodic table
From period the elements in
How does ionic bonding form
Loses an atom from one element and gives to other element to fill outer shell
Does this equation balance na4 + mg +
No
Does this equation balance Na1 + cl-
Yes
How do you represent ionic bonding
Dot and cross diagrams
What structure do ionic compounds have
Regular lattice
Properties of ionic compounds
High melting and boiling points lots of energy required to break strong attraction , don’t conduct electricity because ions are fixed and don’t move but when melted conduct electricity, dissolve in water
How do simple molecules bond
Covalent bonding - share electrons
Properties of simple molecular substances/ covalent bond structures
Low melting and boiling points forced of attraction are very weak. How represent covalent bonds - stick and ball model don’t conduct electricity
What are giant covalent bonds
Many covalent bonds together
Properties of giant covalent structures
High melting and boiling point don’t conduct electricity, even when melted
What are fullerenes
Large carbon molecules
What are nano particles what are they useful for and why
Nano particles are really tiny and have high surface area to volume ratio. This makes them ideal things like deodorant as you can’t see the deodorant and nanomedicine as easy to take
What are nano particles properties and how does this help in real life
Conduct electricity so can be used in tiny chips
Features of metals
High melting and boiling points high density good conductors of heat and electricity bendy
4 structures
Simple covalent, giant covalent, ionic and
Metallic
What does pure mean
Made of one type of compound
How to know if substance is pure or impure
Impure - melting point over range of temperatures
Pure - doesn’t melt over range
What’s formulation
A useful mixture
What does distillation separate
2 liquids or soluble solid from liquid
What does distillation do
Purifies a liquid
What does crystallisation separate
Soluble solid from liquid
What does filtration filtration seperate
Insoluble solid from liquid
What’s the rf formula
Distance by spot/ distance by solvent
What does chromatography seperate
Identifys all the different substance in a mixture
