Chlorine has only one half-filled orbital. This means that it can only bond with one other atom.
In every chlorine atom, there are seven valence electrons.
CH3CO-OH (acetic acid) has 10 valence electrons. The carbon atom contributes 4 valence electrons, each hydrogen atom contributes 1 valence electron, and the oxygen atom contributes 6 valence electrons.
Chlorine has 7 valence electrons.
A molecule shouldn't have valence electrons left.
Seven.
An atom of chlorine has 7 valence electrons because it is in group 17 of the periodic table.
In every chlorine atom, there are seven valence electrons.
A chlorine atom has 7 valence electrons, as it is in group 17 of the periodic table. A chloride ion has 8 valence electrons, as it gains an additional electron to achieve a full octet and a stable electron configuration.
In the question, it should be either "chlorine atom" or "chloride ion". Chlorine atom has 7 valence electrons. Chloride ion has 8 valence electrons.
7, as does an atom of any halogen (element in column 17 of a wide form periodic table.)
There are 7 valence electrons in a chlorine atom. The atomic number of chlorine is 17, which means it has an electron configuration of 2,8,7. This shows it has 3 shells of electrons, with 7 in the outer level.
The element chlorine has seven electrons in its valence shell.
This is a chemical element. You can find the how many electron in a single atom by using a periodic table.
CH3CO-OH (acetic acid) has 10 valence electrons. The carbon atom contributes 4 valence electrons, each hydrogen atom contributes 1 valence electron, and the oxygen atom contributes 6 valence electrons.
Chlorine has 7 valence electrons.
One chlorine atom will form an ionic bond with one magnesium atom. The magnesium will donate its two valence electrons to the chlorine atom, filling both of their valence electron shells.
You would need 1 more electron to make a Chlorine atom stable with 7 valence electrons. This additional electron would allow Chlorine to achieve a full valence shell of 8 electrons, following the octet rule.