ionic compound properties
- have a high melting and boiling point
- they're solid at room temperature
- are hard, but brittle, so they're not malleable or ductile
- don't conduct electricity in solid state
- are good conductors of electricity in liquid state or when dissolved in water
-...
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ionic compound properties
✓ - have a high melting and boiling point
✓ - they're solid at room temperature
✓ - are hard, but brittle, so they're not malleable or ductile
✓ - don't conduct electricity in solid state
✓ - are good conductors of electricity in liquid state or when dissolved in water
✓ - they vary from very soluble to insoluble in water, they're not soluble in non-polar
solvents (oil)
define ionic compounds
✓ made by the chemical combination of metallic and non-metallic elements
nanoscience
✓ the study of nanoparticles and nanotechnology. Nanotechnology is the use of technologies
that manipulate and investigate the properties of materials on the nanoscale.
the prefix nano refers to...
✓ refers to one billionth or 10-9 in scientific notations.
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✓ metal atoms lose electrons to non metallic atoms and become positively charged metal
ions
anions
✓ non metal atoms gain electrons from metal atoms and became negatively charged non
metal ions
what forces result from the attraction between positive and negative charges
✓ electrostatic
explain high melting points of ionic compounds
✓ they have high melting points because a large amount of energy is needed to overcome
the electrostatic attraction between the oppositely charges ions and allow them to move.
So, the ionic bonds between the + and - ions is strong.
explain hardness and brittleness of ionic compounds
✓ a strong force is needed to disrupt the crystal lattice, which means that it's very hard.
Although a salt crystal is hard, a strong force will shatter the crystal, meaning it's brittle.
This is because layers of ions will move relative to each other due to the force of blow.
During this movement, ions of like charge shift so they are next to each other. The
repulsion between the similarly charged ions causes the crystal to shatter
explain electrical conductivity of ionic compounds
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✓ in solid form, ions are held in the crystal lattice and are not free to move, therefore don't
conduct electricity. When solids melt, the ions become free to move, enabling the cations
and anions in the molten compound to conduct electricity. When they dissolve in water,
ionic bonds in the lattice break and the ions are separated and move freely. When an
electric current is applied, + ions move towards the - charged electrode and - ions move
towards the + charged electrodes
properties of metals
✓ Exhibit a range of melting points and relatively high boiling points
✓ Are good conductors of electricity
✓ Are good conductors of heat
✓ Generally have high densities
✓ Are malleable - they can be shaped by beating or rolling
✓ Are ductile - they can be drawn into a wire
✓ Are lustrous or reflective when freshly cut or polished
✓ Are often hard with high tensile strength
✓ Have low ionisation energies and electronegativities
✓
✓ However not all metals have all of these properties
✓ Mercury is a liquid at room temperature (low melting point)
✓ The group 1 elements (the alkali metals) are all soft enough to be cut with a knife and
they react vigorously with water to produce hydrogen gas.
✓ Both mercury and group 1 elements exhibit most of the other properties listed above.
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✓ Transition metals generally have unfilled d-subshells and are often referred to as the d-
block.
✓ Their properties include
✓ They tend to be harder
✓ They have higher densities
✓ They have higher melting points
✓ Some of them have strong magnetic properties
✓ The hardness, higher densities and higher melting points are due to the atoms of transition
metals generally being a smaller size due to their greater core charge. This allows them to
pack together more tightly with stronger bonds
what does each property say about the structure of metals
1. are hard and tend to have high boiling points
2. conduct electricity in solid and molten liquid state
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