Bonding Flashcards
1
Q
Define alloy
A
A mixture of 2 or more metals (may also include nonmetals) to improve its properties.
2
Q
Properties of ionic compounds:
A
- forms between metals and non-metals
- transfer electrons
- strong electrostatic forces of attraction
- giant lattice
- high melting/boiling points
- conducts electricity in molten state
- mostly soluble in water, but not in organic compounds (e.g. benzene, kerosene)
3
Q
Properties of covalent compounds
A
- only forms between non-metals
- sharing electrons
- don’t conduct electricity (no free ions)
- dissolves in organic solvents, but not in water
- low melting/boiling point
- held together by weak Van der Waals forces
4
Q
Define macromolecule
A
Extremely large molecules
5
Q
Describe diamond’s structure and properties
A
- giant tetrahedral macromolecular structure
- very strong covalent bonds
- made up of carbon
- each atom has 4 covalent bonds
- hardest known substance
- atoms can’t slide over each other
- bad conductor (no free electrons)
- high melting/boiling point (due to the sheer number of bonds)
6
Q
Describe graphite’s structure and properties
A
- layered structure, consists of millions of layers
- hexagonal arrangement of carbon atoms
- soft substance
- high melting/boiling point (due to sheer number of covalent bonds)
- can conduct electricity
7
Q
Properties of metallic bonds
A
- metals are electropositive by nature
- atoms in a metal contribute their valence electrons to form a sea of electrons
- electrons float around the positive metal ions, which are arranged in a regular crystal lattice
8
Q
Define metallic bonding
A
The electrostatic attraction between electrons and positive ions in a metal
9
Q
Difference between mixture and compound:
A
While both are used to define two or more elements together, in compounds the elements are chemically combined, while in mixtures the elements are just mixed together.
