Hydrogen-
1
Helium-
0
Lithium-
1
Beryllium-
2
Boron-
3
Carbon-
2, 4
Nitrogen-
3, 5
Oxygen-
2
Fluorine-
1
Neon-
0
Sodium-
1
Magnesium-
2
Aluminium-
3
Silicon-
4
Phosphorus-
3, 5
Sulfur-
2, 4, 6
Chlorine-
1, 3, 5, 7
Argon-
0
Potassium-
1
Calcium-
3, 5
Scandium-
3
Titanium-
3, 4
Vanadium-
2, 3, 4, 5
Chromium-
2, 3, 6
Manganese-
2, 3, 4, 6, 7
Iron-
2, 3
Cobalt-
2, 3
Nickel-
2, 3
Copper-
1, 2
Zinc-
2
Gallium-
2, 3
Germanium-
4
Arsenic-
3, 5
Selenium-
2, 4, 6
Bromine-
1, 3, 5, 7
Krypton-
0
Rubidium-
1
Strontium-
2
Yttrium-
3
Zirconium-
4
Niobium-
3, 5
Molybdenum-
2, 3, 4, 5, 6
Technetium-
2, 3, 4, 6, 7
Ruthenium-
3, 4, 6, 8
Rhodium-
3, 4
Palladium-
2, 4
Silver-
1
Cadmium-
2
Indium-
1, 3
Tin-
2, 4
Antimony-
3, 5
Tellurium-
2, 4, 6
Iodine-
1, 3, 5, 7
Xenon-
0
Caesium-
1
Barium-
2
Lanthanum-
3
Cerium-
3, 4
Praseodymium-
3
Neodymium-
3
Promethium-
3
Samarium-
2, 3
Europium-
2, 3
Gadolinium-
3
Terbium-
3
Dysprosium-
3
Holmium-
3
Erbium-
3
Thulium-
2, 3
Ytterbium-
2, 3
Lutetium-
3
Hafnium-
4
Tantalum-
3, 5
Tungsten-
2, 4, 5, 6
Rhenium-
1, 4, 7
Osmium-
2, 3, 4, 6, 8
Iridium-
3, 4
Platinum-
2, 4
Gold-
1, 3
1, 2
Thallium-
1, 3
Lead-
2, 4
Bismuth-
3, 5
Polonium-
2, 3, 4
Astatine-
1, 3, 5, 7
Radon-
0
Francium-
1
Radium-
2
Actinium-
3
Thorium-
4
Protactinium-
4, 5
Uranium-
3, 4, 5, 6
Neptunium-
2, 3, 4, 5, 6
Plutonium-
2, 3, 4, 5, 6
Americium-
2, 3, 4, 5, 6
Curium-
2, 3, 4
Berkelium-
2, 3, 4
Californium-
2, 3, 4
Einsteinium-
2, 3
Fermium-
2, 3
Mendelevium-
2, 3
Nobelium-
2, 3
Lawrencium-
3
it tells how many electrons are there in an element or compound.
Univalent........table
Univalent 1+
Li
Na
K
A
g
H3o
H
NH4
Cu
Hg
Univalent 1-
F
Cl
Br
I
OH
NO3
HCO3
HSO4
NO2
ClO
MnO4
OCl
H2PO4
-heidikimlinh@Yahoo.com
The Valence is the outer most shell of electrons that an atom will have (2 max per shell).
For example..... S (sulfur) will have 16 electrons and the electrons on that atoms valence will read, 3p4.
Chemical properties
Atomic number Name of element Valency 1 Hydrogen 1 2 Helium 0 3 Lithium 1 4 Beryllium 2 5 Boron 3 6 Carbon 2, 4 7 Nitrogen 3, 5 8 Oxygen 2 9 Fluorine 1 10 Neon 0 11 Sodium 1 12 Magnesium 2 13 Aluminium 3 14 Silicon 4 15 Phosphorus 3, 5 16 Sulfur 2, 4, 6 17 Chlorine 1, 3, 5, 7 18 Argon 0 19 Potassium 1 20 Calcium 3, 5 21 Scandium 3 22 Titanium 3, 4 23 Vanadium 2, 3, 4, 5 24 Chromium 2, 3, 6 25 Manganese 2, 3, 4, 6, 7 26 Iron 2, 3 27 Cobalt 2, 3 28 Nickel 2, 3 29 Copper 1, 2 30 Zinc 2 31 Gallium 2, 3 32 Germanium 4 33 Arsenic 3, 5 34 Selenium 2, 4, 6 35 Bromine 1, 3, 5, 7 36 Krypton 0 37 Rubidium 1 38 Strontium 2 39 Yttrium 3 40 Zirconium 4 41 Niobium 3, 5 42 Molybdenum 2, 3, 4, 5, 6 43 Technetium 2, 3, 4, 6, 7 44 Ruthenium 3, 4, 6, 8 45 Rhodium 3, 4 46 Palladium 2, 4 47 Silver 1 48 Cadmium 2 49 Indium 1, 3 50 Tin 2, 4 51 Antimony 3, 5 52 Tellurium 2, 4, 6 53 Iodine 1, 3, 5, 7 54 Xenon 0 55 Caesium 1 56 Barium 2 57 Lanthanum 3 58 Cerium 3, 4 59 Praseodymium 3 60 Neodymium 3 61 Promethium 3 62 Samarium 2, 3 63 Europium 2, 3 64 Gadolinium 3 65 Terbium 3 66 Dysprosium 3 67 Holmium 3 68 Erbium 3 69 Thulium 2, 3 70 Ytterbium 2, 3 71 Lutetium 3 72 Hafnium 4 73 Tantalum 3, 5 74 Tungsten 2, 4, 5, 6 75 Rhenium 1, 4, 7 76 Osmium 2, 3, 4, 6, 8 77 Iridium 3, 4 78 Platinum 2, 4 79 Gold 1, 3 80 Mercury 1, 2 81 Thallium 1, 3 82 Lead 2, 4 83 Bismuth 3, 5 84 Polonium 2, 3, 4 85 Astatine 1, 3, 5, 7 86 Radon 0 87 Francium 1 88 Radium 2 89 Actinium 3 90 Thorium 4 91 Protactinium 4, 5 92 Uranium 3, 4, 5, 6 93 Neptunium 2, 3, 4, 5, 6 94 Plutonium 2, 3, 4, 5, 6 95 Americium 2, 3, 4, 5, 6 96 Curium 2, 3, 4 97 Berkelium 2, 3, 4 98 Californium 2, 3, 4 99 Einsteinium 2, 3 100 Fermium 2, 3 101 Mendelevium 2, 3 102 Nobelium 2, 3 103 Lawrencium 3
Valency is the amount of electrons available to add or to lose in order to reach a full octet of electrons. For example, Magnesium has a valence of 2. Since there are only two electrons, it would be easier to lose those electrons than to gain more electrons. Therefore, it's electron affinity is low, and its ionization potential is high.
Another example is fluorine. Fluorine has a valence of 7. Naturally it would occur as F2. However, in it's ionic stage as F-, it is highly reactive. It's electron affinity is high (and so is it's electronegativity, meaning it attracts electrons more), and its ionization potential is low.
The main groups of elements (the s and p groups of the periodic table) and their valency can be based on their position. Since there are 7 groups, each one has it's corresponding valency. The first 3 are +. The last 3 are -. I've seen Group 4 elements change all the time. I guess it depends on their isotopes.
All in consideration of Lewis dot diagrams and such.
That is the number of valence electrons, which are he electrons on the outer shell (That can be any shell, not a specific outer shell)
valency is the combining power of an element
The "valency" or valence of an element refers to the number of outermost electrons. It is indicative of the combining power of that element.
The group numbers tell the number of valence electrons. Without looking on the group number you can also tell the number of valence electrons by looking at the highest energy level in the electronic configuration.
Take the atomic number then subtract the amount of valence electrons. Example: Number of non valence (inner) electrons in Sulfur: 16 (atomic number) - 6 (valence electrons) = 10 (valence or inner electrons)
Hydrogen has a valence of 1.
Group 2 metals have 2 valence electrons. In fact, the number of valence electrons of elements can be deduced from the group number (e.g. group VII elements have 7 valence electrons).
3 electrons !
its a valence number which is and above
the number of valence electrons is the number group on the table its on
Take the atomic number then subtract the amount of valence electrons. Example: Number of non valence (inner) electrons in Sulfur: 16 (atomic number) - 6 (valence electrons) = 10 (valence or inner electrons)
The group numbers tell the number of valence electrons. Without looking on the group number you can also tell the number of valence electrons by looking at the highest energy level in the electronic configuration.
Take the atomic number then subtract the amount of valence electrons. Example: Number of non valence (inner) electrons in Sulfur: 16 (atomic number) - 6 (valence electrons) = 10 (valence or inner electrons)
Hydrogen has a valence of 1.
Two valence electrons.
The expected number of valence electrons for a group 3 A element is 5 number of valence electrons.
2 is the standard number of valence electrons
It has 4 valence electrons and a valence electron potential of 95.2
Valence electrons and group number for metal are same. For non-metals, valence electrons are equal to group number-10.
They don't have the same number. that's what makes thme all different