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The way in which elements bond to form compounds depends on the arrangement and number of electrons in the atoms. This is what will determine the type of boding that elements will form.
Five valence electrons. They all exhibit different oxidation numbers too!!!!
Valence is how many bonds an atom can form. Oxidation number can be though of as being similar to the charge on an ion, and is based on the difference in electronegativity between bonded atoms. If something is bonded to a more electronegative element, its oxidation state is positive, and if it is with a less electronegative on the state is positive. In a neutral substance the sum of the oxidation states is always zero. Valence and oxidation states are related, though.Example: In formaldehyde (CH2O) hydrogen has a valence of 1, oxygen a valence of 2, and carbon a valence of 4. Carbon is more electronegative than hydrogen, and less electronegative than oxygen. As a result, each hydrogen atom has an oxidation state of 1+ and the oxygen is in the 2- oxidation state. This puts carbon in an oxidation state of 0.
Oxidation number of F is -1.Oxidation number of O is +2.
Group 1 elements are the most electropositive in nature and have only 1 valence electron. So, they always show the oxidation state of +1.
It indicates how many electrons are required to complete a full valence shell.
Because they have one valence electrons, and if they lose this electron they attain an oxidation number of +1
Because they have the same characeristics such as the oxidation states or the valence.
The way in which elements bond to form compounds depends on the arrangement and number of electrons in the atoms. This is what will determine the type of boding that elements will form.
The Roman numeral in the parentheses is the valence or oxidation of the metal that it follows. Transition elements have more than one oxidation number
Five valence electrons. They all exhibit different oxidation numbers too!!!!
Valence is how many bonds an atom can form. Oxidation number can be though of as being similar to the charge on an ion, and is based on the difference in electronegativity between bonded atoms. If something is bonded to a more electronegative element, its oxidation state is positive, and if it is with a less electronegative on the state is positive. In a neutral substance the sum of the oxidation states is always zero. Valence and oxidation states are related, though.Example: In formaldehyde (CH2O) hydrogen has a valence of 1, oxygen a valence of 2, and carbon a valence of 4. Carbon is more electronegative than hydrogen, and less electronegative than oxygen. As a result, each hydrogen atom has an oxidation state of 1+ and the oxygen is in the 2- oxidation state. This puts carbon in an oxidation state of 0.
Oxidation number of F is -1.Oxidation number of O is +2.
Group 1 elements are the most electropositive in nature and have only 1 valence electron. So, they always show the oxidation state of +1.
It indicates how many electrons are required to complete a full valence shell.
They share the same number of electrons (=2) in the valence shell: they have the same oxidation state of +2
it indicates how many electrons are required to complete a full valence shell