Silicon is in Group 14, and all members of Group 14 have 4 electrons in the outermost energy level, or valence shell (14-10). Also, silicon is in the second column of the p-block on the Periodic Table. All members of the p-block have a valence shell of ns2np1-6, where n is the outermost, or highest energy level. Since silicon is in the second column of the p-block, and it is in period 3, its electron configuration is [Ne]3s23p2, in which the outermost, or highest energy level, or valence shell is the 3rd energy level, which contains 4 electrons.
The number of protons and electrons is specific for atoms in a neutral state.
Elements are arranged into rows in order of increasing mass, so that elements with similar properties were in the same column. They are organized by type, such as nonmetals, metals, and metalloids, and solids, liquid, gas, or not found in nature.
Iodine is a halogen (group 7 of the periodic table), and halogens are supposed to have seven valenced electrons to match the amount of protons in their nucleus. However, in order to form a full octet of valence electrons, iodine atoms are willing to accept one more electron. This electron brings iodine's charge down to -1. And unlike other halogens that are smaller than iodine (fluorine, chlorine, and bromine), iodine is large enough so that its negative charge can be distributed more evenly. This makes iodine stable with a negative charge, and a good leaving group in chemical reactions (something you will probably learn later on in organic chemistry).
Basically, electricity is a force caused by electrons hitting each other. The electron sea model explains the conductivity of transition metals by showing that they hang onto their many electrons loosely and are practically floating in them. With so many free electrons, it's a lot easier to conduct electricity.
If you know the atomic no. and atomic mass, then the no. of electrons, no. of protons and no. of neutrons can also be determined. Atomic No.=No. of electrons = No. of protons. No. of neutrons=Atomic mass-Atomic no. Also, by no. of electrons you can determine its valency and the no. of valence electrons.
The position in the periodic table can range in size moving from left to right, and it has a wider range of numbers, but in the outermost suborbital, it can only range from 1-8 valence electrons!
the group number shows the number of electrons in the outermost energy levels. forexample sodium (Na) have 1 electron in the outermost shell and is placed in the group 1. Elements are grouped in rows depending on their energy levels, or valence electron numbers. Columns of elements are those that are chemically similar, or react
atomic no. or basically according to the no. of electrons in their outermost shell whcih reflect the property of individual atom
Alkali metals are positioned to the far left in the periodic table. They react with hydrogen and oxygen(no they don't react with metals) and they have one electron in the outermost orbit.Halogens are positioned next to the noble gases in the periodic table. They react with nonmetals (no they don't react with metals) and they have seven electrons in the outermost orbit.Noble gases are positioned to the far to the right or last column in the periodic table. They never react with metals (no they don't react with metals) and they have 0 electron in the outermost orbit because they are very unreactive, which mean they are neutral (0/canceled).***Bold Words Important Keys for the Words***(Answers are found in page #110, 111, and 112 in the Grade 9 Nelson Science Textbook for Ontario, and also use the modern periodic table as your guide.)
Electrons in the outer most energy level is called "valence electrons." Groups are the columns of the periodic table. The more valence electrons (up to 8), the closer to the right. The number of electrons needed to make an atom stable is 8. (Minus Hydrogen and Helium, which only need 2 electrons to be stable.)
i think it tells about the stability of that element.add The position and number of electrons on an element determine its chemical properties. Generally, the outermost shell of electrons.But in the rare earths, the outermost shell of all of them, contains a similar number of electrons, and it is the inner shells that vary in their number. Hence their similar but subtly different properties.
it is in group, 4 and in period 2 group means how many electrons in outer shell, and period means how many electron shells it has:)
Position of Periodic Table describes chemical properties. it is estimated from its position in table.
The group number is found by the number of valence electrons. The period number is found by the number of energy levels. These 2 controls the position of an element.
The model is applied to movement and position of electrons in the atom.
2, as indicated by its position in periodic column 2.
how many electrons it has---how many valence electrons and how many levels of electrons. its Atomic Mass its atomic number