3.2/3 ATOMIC STRUCTURE + IONIC BONDING Flashcards
Define an isotope
Atoms of the same element, that have a different number of neutrons but same number or protons and electrons.
How do different isotopes affect the chemical and physical properties of an atom
It has the same chemical properties, but the melting point and density are different
What happens to the electrons in a metal ion
They lose electrons to give it a positive charge
What happens to the electrons in a non-metal ion
They gain electrons to give it a negative charge
What is reduction in ions
Gain of electrons
What is oxidation in ions
Loss of electrons
How do you calculate the relative atomic mass
1) Multiply the abundances by the mass and divide by 100
2) Do the same for all the isotopes.
3) Add them together
Define ionic bonding
The strong electrostatic attraction between oppositely charged ions
What are the relative masses and relative charges of the subatomic particles
Proton- 1
Neutron- 1
Electron- 0.001
What does the atomic number tell you about an atom
The number of protons
What does the mass number tell you about an atom
The number of protons and neutrons
What is a cross on a dot and cross diagram
The electrons the atom already has
What is a dot on a dot and cross diagram
The electrons it has gained
How do you draw a dot and cross diagram
1) Draw out all the atoms needed
2) Draw arrows from outer shell electrons from the metal to the outer shell electrons of the non-metal
3) Draw an arrow labeled ion on it
4) In brackets, draw the newly formed ions with the relevant electrons in crosses and dots with the charge outside the brackets in the top right corner and shell configuration on the bottom
How are ionic compounds arranged
A giant ionic lattice layered
Why do ionic compounds have high melting points
1) The ionic bonds are very strong
2) In a giant ionic lattice there are lots of ionic bonds
3) Breaking all the ionic bonds requires a large amount of energy
How does the charge of ions in the giant ionic lattice affect the strength of the structure
The more charge in the ions, the stronger the giant ionic lattice
Why aren’t solid ionic compounds conductors
The electrons aren’t free to move
Why can ionic compounds conduct as a liquid
The electrons are free to move
Why do ionic compounds conduct electricity when molten or dissolved but not solid
1) When solid, the ions are fixed and not free to move , so they cannot carry charge or flow
2) When they are dissolved or molten the ions are free to move allowing charge to flow therefore becoming conductive
Are ionic substances soluble in water
Usally
Describe the visual appearance of an ionic compound
Crystalline
Are ionic substances brittle or malleable
Brittle
