EL 8 Spectacular Metals Flashcards
Physical Properties of Metals (9)
- Malleable
- Sonorous
- High Density
- Shiny
- Ductile
- Good Thermal Conductor
- Good Electrical Conductor
- High Melting Point
- High Boiling Point
Explain bonding in metals [3 marks]
- Metallic Bonding
- The outer electrons of metals become delocalised and are free to move in a sea of electrons
- Positively charged metallic cations are attracted to the delocalised negatively charged electrons
Group 1 and 2 Metal Properties (3)
- Soft = Easy to cut
- Weak = Breaks easily
- Low melting point
Group 1 and 2 Metal Origins (What are they found as)
- Highly reactive = Found as cations (Positively charged ions)
Define “salt”
A chemical compound consisting of an ionic assembly of positively charged cations and negatively charged anions
Group 1 and 2 Metals react with water to form…?
Metal + Water —> Metal Hydroxide and Hydrogen
Group 1 Metals are known as…?
Alkaline Metals
Group 2 Metals are known as…?
Alkaline Earth Metals
Hydroxide Ion
OH 1-
Nitrate Ion
NO3 1-
Sulphate Ion
SO4 2-
Carbonate Ion
CO3 2-
Hydrogen Carbonate Ion
HCO3 1-
Group 1 and 2 Metals react with oxygen to form…?
Metal + Oxygen —> Metal Oxide
Group 1 and 2 Metals react with halogens to form…?
Metal + Halogen —> Metal Halide
Why are Group 1 and 2 Metals more reactive as you go down? (3)
i) Greater Number of Shells
ii) Electron Shielding
iii) Greater Nuclear Charge
Why are Group 1 Metals more reactive than Group 2 Metals?
Group 1 = 1 electron to be removed
Group 2 = 2 electrons to be removed
Therefore, Group 2 requires more energy = less reactive
Group 2 Metal Oxides react with water to form…?
Metal Oxide + Water —> Metal Hydroxide
Group 2 Metal Oxides react with acid to form…?
Metal Oxide + Acid —> Salt + Water
Group 2 Metal Hydroxides react with acid to form…?
Metal Hydroxide + Acid —> Salt + Water
Group 2 Metal Hydroxides dissolve in water to form…?
Metal Hydroxide —-> Metal Ions + Hydroxide Ions
Factors affecting Charge Density (2)
- Ions with a smaller radius = higher charge density
—> i.e. found at the top of groups in the periodic table - Ions with a greater charge = higher charge density
—> Al3+ > K+
Group 2 Carbonates Thermal Stability Trend
As you go down Group 2, thermal stability increases (requires more heat) since there is less distortion
Group 2 Hydroxides Solubility Trend
As you go down Group 2, solubility increases
Group 2 Sulphates & Carbonates Solubility Trend
As you go down Group 2, solubility decreases
Define First Ionisation Enthalpy
The energy requires to remove one electron from every atom in one mole of isolated gaseous atoms
First Ionisation Enthalpy Equation
X(g) —> X+(g) + e-
Shape of a s subshell
Spherical
Number of orbitals in a s subshell
One Orbital
Shape of a p subshell
Dummbell
Number of orbitals in a p subshell
Three Orbitals
Shape of a d subshell
Double Dummbell
Number of orbitals in a d subshell
Five Orbitals
How many electrons can fit in a single orbital?
2e-
Factors which affect Ionisation Enthalpy (3)
i) Atomic Radius
Larger radius = Less energy required
ii) Electron Shielding
More shields lead to more shielding = Less energy required
iii) Nuclear Charge
The number of protons in the nucleus influences the Ionisation Energy
Why is there a drop in Ionisation Energy between Group 2 and 3?
The addition of a p subshell
Why is there a drop in Ionisation Energy between Group 5 and 6?
The electron repulsion when the 4th electron occupies its position in the orbital
Thermal Decomposition of a Metal Carbonate
MCO3(s) —> MO(s) + CO2(g)
Group 2 Hydroxide’s pH in Water Trend
As you go down Group 2, pH increases
As you go across a Period, what happens to the Ionisation Energy and why is this?
Number of Shells and Shields stay the same = These factors have no effect on the Ionisation Energy
Nuclear Charge Increases = Ionisation Energy generally increases
Example : Why is AlCl3 more distorted than NaCl?
The cation Al 3+ has a greater charge than that of the cation Na +, therefore Al 3+ has a higher charge density than Na +
Example : Why is AlF3 less distorted than AlBr3?
The anion F- has a smaller radius than that of the anion Br-, therefore Br- has a lower charge density and is more readily distorted
