c7 flashcards test
(14 cards)
What type of compounds were primarily discussed in the naming and bonding table?
Ionic compounds
Ionic compounds consist of a metal and a non-metal, where electrons are transferred from the metal to the non-metal.
What are the products of the complete combustion of heptane?
Carbon dioxide and water
The reaction is: C₇H₁₆ + 11O₂ → 7CO₂ + 8H₂O.
What occurs during incomplete combustion of pentane?
Production of carbon monoxide or carbon and water
The reactions are: C₅H₁₂ + 5O₂ → 5CO + 6H₂O or C₅H₁₂ + 3O₂ → 5C + 6H₂O.
What is the classification of mercury and why?
Metal
Mercury conducts electricity due to delocalised electrons and is liquid at room temperature.
What is the structure of silicon carbide (SiC) and its properties?
Covalent network solid
SiC has a giant lattice structure with strong covalent bonds, giving it exceptional hardness and thermal stability.
What is shown in the Lewis dot structure of carbon monoxide (CO)?
A triple bond between carbon and oxygen
Each atom has one lone pair, and oxygen donates a lone pair to form a coordinate covalent bond.
What determines the number of electrons gained, lost, or shared when two elements form a compound?
Valency
Valency indicates how elements interact in forming covalent or ionic compounds.
What type of reactions do saturated hydrocarbons (alkanes) undergo?
Substitution reactions
These reactions are generally slow and require UV light to initiate.
What type of reactions do unsaturated hydrocarbons (alkenes and alkynes) undergo?
Addition reactions
These reactions are faster and do not require catalysts or light.
What are intermolecular forces?
Forces of attraction between molecules
Includes dispersion forces, dipole-dipole interactions, and hydrogen bonding.
List the four allotropes of carbon.
- Diamond: covalent network solid, extremely hard, non-conductive
- Graphite: layered structure, good conductor, slippery
- Fullerene (C₆₀): spherical molecular structure, low melting point
- Graphene: single layer of graphite, highly conductive and strong
What are valence electrons?
Outermost electrons involved in bonding
Atoms gain, lose, or share these electrons to achieve a full outer shell.
Why are metals ductile?
Atoms are arranged in layers that can slide over one another
Delocalised electrons allow layers to move without breaking bonds.
Why are gases considered volatile?
Particles are far apart with weak intermolecular forces
Gases require little energy to escape into the gas phase and readily evaporate.
