What is the naming convention for ionic compounds involving a metal and a nonmetal?
- Metal name unchanged
- Nonmetal ends in –ide
- Transition metals use Roman numerals
- Polyatomic ions keep their names
Example: Al³⁺ + O²⁻ → Al₂O₃
What are the steps for writing the formulas of ionic compounds?
- Write charges
- Criss-cross
- Reduce subscripts
Example: Al³⁺ + O²⁻ → Al₂O₃
What prefixes are used in the naming of covalent compounds?
- mono
- di
- tri
- tetra
- penta
- hexa
- hepta
- octa
- nona
- deca
Example: CO₂ = carbon dioxide
In naming covalent compounds, when is a prefix used for the first element?
Only if >1
The second element always uses a prefix + –ide.
What is the formula representation for dinitrogen monoxide?
N₂O
Prefixes in covalent compounds equal subscripts.
What is the naming convention for binary acids?
- Starts with “hydro”
- Change ending of second element to -ic
Example: HCl —> hydrochloric Acid
How do you name polyatomic acids when the ion ends with -ate?
Change to -ic
Example: HNO3 —> Nitric Acid
How do you name polyatomic acids when the ion ends with -ite?
Change to -ous
Example: HNO2 —> Nitrous Acid
What are the properties of ionic compounds?
- Electron transfer
- High melting/boiling points
- Conduct when molten or dissolved
- Usually solids
- Often water-soluble
- Strong electrostatic attraction
Ionic compounds are characterized by their distinct properties.
What are the properties of covalent compounds?
- Electron sharing
- Can be solid/liquid/gas
- Low melting/boiling points
- Do not conduct electricity
- Often not water-soluble
- Distinct molecular shapes
Covalent compounds exhibit different physical and chemical properties compared to ionic compounds.
What are the characteristics of acids?
- Produce H⁺ ions in water
- pH < 7
- Sour taste
- Turn blue litmus → red
- Corrosive
- Conductive (ionization)
- React with metals → H₂ gas
Acids have specific properties that distinguish them from other substances.
