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What else can I help you with?
How do you determine the charges of a sulphur ion on the periodic table?
The most common ion is S2-.
Which element is located in the family represented by n s2 n p 3?
The elements with a s2 p3 electron configuration are located in the 5A (or 15) column of the periodic table: nitrogen, N; phosphorus, P; arsenic, As; antimony, Sb, and bismuth, Bi.
What can you predict about an element by its position on the periodic table?
By the position of an element on the periodic table you can tell how many protons the element has in it by looking at the number above the elements symbol. You can also find the electron configuration with that same number then you can and you can you can also tell if it is f1, f2,f3...s1,s2,d1,d2...
Using the periodic table predict the charge of a sulfide ion?
A sulfide ion will have a charge of -2. This is because sulfur is in Group 6 of the periodic table and typically forms ions by gaining two electrons to achieve a stable, noble gas electron configuration.
Which is bigger o 2 ion or s 2?
S^2- is larger in size compared to O^2-. This is because sulfur is lower in the periodic table than oxygen, and as we move down a group in the periodic table, the atomic size generally increases.
Which group will have an electron configuration that ends in s2?
Elements in Group 2 of the periodic table will have an electron configuration that ends in s2. This group includes elements such as beryllium, magnesium, and calcium. They have two electrons in their outermost s sublevel.
What atom in row 3 of the periodic table is likely to form a -2 ion?
The atom in row 3 of the periodic table that is likely to form a -2 ion is sulfur (S). Sulfur is in group 16 and can gain two electrons to achieve a stable electron configuration.
What ions are formed with magnesium and sulfur?
Magnesium is located in Group II in the periodic table. Every element in Group II will form an ion with the charge of 2+ by losing two electrons. Hence, magnesium will form the magnesium ion: Mg2+. Sulfur is located in Group VI in the periodic table. Every element in Group VI will form an ion with the charge of 2- by gaining two electron. Hence, sulfur will form the sulfur ion: S2-.
What is the noble gas notation of the element with valence electron s2?
S2- ion: [Ne]3s23p6
How do you explain superset?
Definition: A set S1 is a superset of another set S2 if every element in S2 is in S1. S1 may have elements which are not in S2.
How is the periodic table set up?
If you do a chemistry degree you will likely have entire modules revolving around this and various trends. The periodic table is actually set up extremely carefully and cleverly. I'll give a quick overview. 4 Blocks: S Block - (Columns 1 and 2) - Valence electrons of elements is in the S orbital. D Block - (Columns 3 - 12) - Valence electrons of elements is in the D orbital. P Block - (Columns 13 - 18) - Valence electrons of elements is in the P orbital. F Block - (Those 2 rows at the bottom, separate) - Valence electrons in F orbital. And that makes sense. S shell holds 2 electrons, it has 2 columns. P shell holds 6 electrons, gets 6 columns and etc etc. So now we can see that S block column 2 has valence S2. Row 6 is P block. Valence is s2, p4. Total of 6 electrons. Since we can tell a LOT about an element's properties from its valence electrons, a glance at the periodic table proves to be extremely useful. The more you use it, the more obvious the trends become. We also get trends like electronegativity increasing toward the top right...and a hundred other trends, again it only takes a quick look at the periodic table to gain important knowledge. The rows, usually numbered down the left-side of the table show us what number our valence shell is (tells us the principle quantum number of the valence shell, n). For example: Vanadium is in D block. It's in group 5 and row 4. Right away I know Vanadium has 3d3 4s2 valence. D-Blocks have funny little quirks with how their shells fill but don't worry too much about that. Practice a few and it'll become very easy. The F-Block is kept well out of the way, which is a good idea considering they are generally less used...but more importantly, it keeps the table in a useful format. Plus it groups the F-Block together, which share some chemical properties and can be useful to view as a separate group. In almost any chemistry subject you do, there WILL be trends relating to it on the periodic table, just look for them. And good chemists can do huge amounts of work with atoms they know nothing about, using just the periodic table and some know-how.
A member of the same family as oxygen whose most stable ion contains 18 electrons?
The element that fits this description is sulfur. Its most stable ion is the sulfide ion (S2-), which contains 18 electrons. Sulfur belongs to the same group as oxygen on the periodic table (Group 16 or 6A), known as the chalcogens.
