Structure + Bonding Flashcards
Elements with the … Number of electrons on the … Shell have … … Properties
Same
Outer
Similar
Chemical
How are ions similar and different in the periodic table
Similar: react the same because same electrons in outer shell
Different: react different because more shells down the group in group 1
The relationship between group number and electronic configuration is shown in the table
Group | no electrons out shell | ion charge 1 1 +1 2 2 +2 3 3 +3 4 4 X 5 5 -3 6 6 -2 7 7 -1 8 2/8 X
The element in group 4 and 8(0) generally do not…
Form ions
Noble gases are unreactive because their atoms …
Have stable electronic arrangements
Atoms other than noble gases can achieve stable electronic structures by … Or … Electrons to form ions ( or … Electrons to form … Bonds)
Gaining
Losing
Sharing
Covalent
Positive and negative ions … To form … Bonds
Attract
Ionic
Ionic bonds hold … Charged ions together in … Structures. Strong electrostatic forces of attraction act in … Directions.
Oppositely
Giant
All
Each ion in the lattice is … By ions with the … Charge and so is held … In place
Surrounded
Opposite
Firmly
Draw a sodium chloride crystal
On paper
A lot of … is needed to … the ionic bonds to melt the solids so ionic compounds have … melting and boiling point
Energy
Overcome
High
… ionic compounds … conduct electricity as the ions are held firmly in place by strong electrostatic forces
Solid
Cannot
When ionic compounds are … in water the ions are … from one another by the water molecules. They are then … to move in solution, are able to … charge and therefore able to … electricity.
Dissolved Separated Free Carry Conduct
When ionic compounds are melted they are … To conduct electricity as the ions are … To move and are able to … Electrical charge
Able
Free (sea of delocalised electrons)
Carry
What is the representation of a sodium chloride called
Giant lattice structure
Giant Covalent bonding
- Non metal to non metal
- these structures contain many strong covalent bonds (diamond)
- high melting points
- doesn’t conduct electricity
- not soluble in water
Ionic bonding
- Non metal to metal
- gaining or losing electrons to achieve a full outer shell
- high melting points
- cannot conduct electricity
- soluble in water
Metallic bonding
- Metal to metal
- lattice structure of metal ions with outer shell electrons free to move through the structure
- high melting point
- conducts electricity
- not soluble in water
Covalent bonding is the … Of attraction between a… And the … Of the adjacent atoms
Electrostatic force
Shared pair of electrons
Nucleus
Strong covalent bonds exist between atoms to form … molecules. The force of attraction between these molecules is very weak (AKA …) things that have low melting points have a … covalent bond.
Small
Intermolecular forces of attraction
Simple
Name 3 properties, uses and the structures of graphite
- Layers slide over each other, lubricant and pencil lead, forms flat sheets of covalently bonded structures which are stacked on top of each other but held together by weak non covalent interactions
- conducts electricity, electrodes, as there is a vast delocalisation within the carbon layers which have free electrons so are able to conduct electricity
- very high melting point, crucible for holding molten metal, the bonds holding together the layers (intermolecular bonds) are very strong and requires a lot of energy to separate
Name 3 properties, uses and structures of a diamond
- doesn’t conduct electricity, insulating material, no free electrons to carry electricity current as all of its valence electrons are involved in bonding
- hardest material known, cutting tools and drills, has most stable atomic structure which makes it more difficult to remove molecules
- very high melting point, jewellery, strong carbon covalent bonds which is considered as a stone with superlative physical qualities as contains bonds which are extremely hard to break
Diamonds and graphite both only contain … And are … Of each other
Carbon
Allotropes
Metallic bonding properties
- high melting and boiling points: as they have powerful attractions so a lot of energy is required to separate them
- conduct electricity: this is because the delocalised electrons are free to move throughout the structure
- malleable: easily beaten into shape
- ductile: easily pulled into wires
Simple molecular (covalent) bonding
- non metal to non metal
- electrostatic force of attraction between a shared pair of electrons
- low melting points
- cannot conduct electricity
- insoluble
Cation and anion difference
Cation is positive
Anion is negative
Hydroxide charge and symbol
-1
OH
Nitrate charge and symbol
-1
NO3
Carbonate charge and symbol
-2
CO3
Sulphate charge and symbol
-2
SO4
Sulphite charge and symbol
-2
SO3
Solid structure
Tight, uniform, small vibrations, strong forces of attraction between them
Liquid structure
Moulds to its container, particles still touching a bit with some gaps, less dense than solids, forces of attraction are weaker
Gas structure
Very far apart, not uniform structure, basically no forces of attraction between them
When a solid turns to liquid
Melts at its melting point, vibrations become stronger an stronger until forces of attraction are no longer strong enough to hold them together
When a liquid turns to a gas (evaporation)
Some fast particles on the surface of the liquid will have enough energy to break away from the gas
When a gas turns to a liquid
Condensation, when gas is cooled the particles eventually move slowly enough that attractions between them hold as a liquid
When a liquid turns to a solid
Solidification, particles start to move slowly until so slow that forces of attraction can hold them together in a solid
Solid to gas and vice versa
Sublimation, no ability to be in a liquid state
When a liquid turns to a gas (boiling)
When the liquid is heated so strongly that the particles are moving fast enough to break all forces of attraction, bubbles of gaseous particles are formed throughout the liquid and rise to the surface
A gas can diffuse between others, describe it vertically and horizontally
Vertically - quickly if denser gas on top
Horizontally - slowly and diffuse not in the middle but on the side of denser gas
Dilution of strongly coloured solution like potassium manganate and water
Takes days for the colour to diffuse throughout the whole water as only smalls gaps between the liquid particles for other particles to diffuse into
Diffusion of bromine particles and air
Can diffuse very easily, the brown colour will diffuse upwards or sideways until all the colours are light brown, boh particles bounce around constantly to give an even mixture
Define an atom
the smallest component of an element having the chemical properties of the element, consisting of a nucleus containing combinations of neutrons and protons and one or more electrons bound to the nucleus by electrical attraction; the number of protons determines the identity of the element.
Define a molecule
the smallest physical unit of an element or compound, consisting of one or more like atoms in an element and two or more different atoms in a compound.
Define an element
one of a class of substances that cannot be separated into simpler substances by chemical means
Define a compound
a pure substance composed of two or more elements whose composition is constant.
Define a mixture
two or more substances that are not chemically united and that exist in no fixed proportion to each other
Atom structure
Nucleus made up of protons and neutrons
Electrons found in large distance from the nucleus orbiting it
Relative charge and mass for a neutron
Charge - 0
Mass - 1
Relative charge and mass for an electron
Charge - -1
Mass - 0
Relative charge and mass for a proton
Charge - +1
Mass - 1
