4. click on al and s\natom\tvalence electrons\tmetal or nonmetal\thow many of each atom is required to form…
4. click on al and s\natom\tvalence electrons\tmetal or nonmetal\thow many of each atom is required to form the compound?\nal\t\t\ns\t\t\nwhat type of bond does al and s form (ionic or covalent/molecular)?\nwhat is the formula?\twhat is the name?\n5. click on o and cl\natom\tvalence electrons\tmetal or nonmetal\thow many of each atom is required to form the compound?\no\t\t\ncl\t\t\nwhat type of bond does o and cl form (ionic or covalent/molecular)?\nwhat is the formula?\twhat is the name?\n6. click on ca and f\natom\tvalence electrons\tmetal or nonmetal\thow many of each atom is required to form the compound?\nca\t\t\nf\t\t\nwhat type of bond does ca and f form (ionic or covalent/molecular)?\nwhat is the formula?\twhat is the name?\nsummarize the rules for naming ionic and covalent compounds here: 1. decide if ionic vs. covalent by \na. if ionic, then use the name of the metal ion (or positive ion) followed by the name of the negative ion)\nb. if covalent, then use the names of each element with an ending the 2nd element, and use to tell how many each atom you have.
Answer
Explanation:
Step1: Determine properties of Al and S
Al (aluminum) has 3 valence electrons, is a metal. S (sulfur) has 6 valence electrons, is a non - metal. To form a compound, we need 2 Al atoms and 3 S atoms to balance the charges. They form an ionic bond. The formula is $Al_2S_3$ and the name is aluminum sulfide.
Step2: Determine properties of O and Cl
O (oxygen) has 6 valence electrons, is a non - metal. Cl (chlorine) has 7 valence electrons, is a non - metal. They form a covalent bond. To form a stable compound, we can have different combinations like in $Cl_2O$ (dichlorine monoxide), $ClO_2$ (chlorine dioxide) etc. For simplicity, if we consider $Cl_2O$, we need 2 Cl atoms and 1 O atom.
Step3: Determine properties of Ca and F
Ca (calcium) has 2 valence electrons, is a metal. F (fluorine) has 7 valence electrons, is a non - metal. They form an ionic bond. We need 1 Ca atom and 2 F atoms to form $CaF_2$, named calcium fluoride.
Step4: Naming rules
To decide if ionic or covalent: If a metal and non - metal combine, it is ionic. If two non - metals combine, it is covalent. For ionic compounds, use the name of the metal ion followed by the name of the negative ion. For covalent compounds, use the names of each element with an appropriate prefix for the second element, and use prefixes to tell how many of each atom you have.
Answer:
| Atom | Valence Electrons | Metal or Nonmetal | How many of each atom is required to form the compound? |
|---|---|---|---|
| Al | 3 | Metal | 2 |
| S | 6 | Nonmetal | 3 |
| O | 6 | Nonmetal | 1 (in $Cl_2O$) |
| Cl | 7 | Nonmetal | 2 (in $Cl_2O$) |
| Ca | 2 | Metal | 1 |
| F | 7 | Nonmetal | 2 |
Type of bond for Al and S: Ionic Formula for Al and S: $Al_2S_3$ Name for Al and S: Aluminum sulfide
Type of bond for O and Cl: Covalent Formula for O and Cl (example): $Cl_2O$ Name for O and Cl (example): Dichlorine monoxide
Type of bond for Ca and F: Ionic Formula for Ca and F: $CaF_2$ Name for Ca and F: Calcium fluoride
Naming rules:
- Decide if ionic vs. covalent by checking if a metal and non - metal combine (ionic) or two non - metals combine (covalent) A. If ionic, then use the name of the metal ion (or positive ion) followed by the name of the negative ion) B. If covalent, then use the names of each element with an appropriate prefix for the 2nd element, and use prefixes to tell how many of each atom you have.