Group 1 Chemical Properties: Forming Cations | Alkali Metals | GCSE Chemistry (9-1) | kayscience.com
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Alkali metals form stable cations with a 1+ charge by losing one electron, exhibiting similar chemical properties due to metallic bonding. By analyzing the periodic table, one can determine the type of bonding in a substance based on the elements present: metallic bonding for metals, ionic bonding for metal-nonmetal compounds, and covalent bonding for nonmetals.
Insights
- Alkali metals in group one of the periodic table have increasing mass numbers down the group, resulting in larger atoms with similar chemical and physical properties due to metallic bonding.
- Group one metals form stable cations with a 1+ charge by losing one electron, showcasing a pattern in their electron configurations that leads to the creation of full outer electron shells.
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What are alkali metals?
Group one metals located on the far left.
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Summary
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Alkali Metals: Properties, Bonding, and Cations
- Group one metals, known as alkali metals, are located to the far left of the periodic table and include lithium, sodium, potassium, rubidium, cesium, and francium. The mass number increases as you move down the group, leading to larger atoms. Alkali metals exhibit similar chemical and physical properties due to metallic bonding.
- Alkali metals react with nonmetals to form ionic compounds with ionic bonding. By examining the periodic table, one can determine the type of bonding in a substance based on the elements present: metallic bonding for metals, ionic bonding for metal-nonmetal compounds, and covalent bonding for nonmetal substances.
- Group one metals lose one electron to become stable cations with a 1+ charge. This process is illustrated by the electron configurations of lithium, sodium, and potassium, showing how each element forms a cation by losing an electron to achieve a full outer shell of electrons.
