It would need to ionize, by combing with another fluoride atom.
Draw the nucleus. Add three obits or rings. Put 2 electrons in the first orbit (filling it). Put 8 in the second orbit (filling it) and 7 in the third. There should be 8 to fill this but there isn't so chlorine is reactive: "looking" to fill the third orbit.
One electron is needed.
There are an infinite number of excited states that fluorine's 9 electrons could be in. To write one you simply need to write out the excited state of fluorine and put one of its electrons in a higher energy orbital. F: 1s2 2s2 2p5 F*: 1s2 2s1 2p5 3s1 The latter is just one possible excited state of fluorine.
An atom of fluorine has 9 electrons in total. Electrons are equal to protons when the atom isn't an ion, and the number of protons is also the atomic number of the element, so you just need to know the atomic number to find out the number of electrons or protons.
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Berilium, Magnesium, Calcium, Strontium, Barium and Radium
One
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Fluorine and chlorine both need to gain electrons in order to achieve a stable electron configuration of 8 electrons in their outer shell, but fluorine is the smaller atom. As atoms get larger, their ability to attract electrons is reduced and they become more metallic in nature and less nonmetallic, because the outer shells of the electrons are farther from the positively charged nucleus, and even though the nucleus of larger atoms also has a larger positive charge, the increase in charge has less effect than the increase in distance, because charge is a direct proportionality and distance is an inversely squared proportionality. Distance matters more. So fluorine has the greater attraction for electrons, or as you put it, it has the greater reduction potential.
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Oxygen have 6 electrons on the outer sell so it need 2 more electrons to gain full outer shell. Magnesium have 2 electrons on the outer sell so It have to lose 2 electrons to gain full outer sell. They combine easily by a strong ionic bond. Its formula is MgO, it has no overall charge.
Draw the nucleus. Add three obits or rings. Put 2 electrons in the first orbit (filling it). Put 8 in the second orbit (filling it) and 7 in the third. There should be 8 to fill this but there isn't so chlorine is reactive: "looking" to fill the third orbit.
1
Carbon has four valence electrons, so it will need four more electrons to fill its outer shell.
These electrons are called "outershell electrons" or "valence electrons."
That depends on the reaction, and the gain of electrons is refereed to as reduction.
It depends, most atoms need 8 total valence electrons in their outer shell (some need 2). So subtract the number they have (determined by the group that the element is in) from 8 and that is how many they need to fill their outer shell!