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What is the trend in the number of valence electrons as you move down a group?
Wiki User
∙ 13y ago
There is no trend for going down a group. The only trend is that valence electrons increase from left to right, across a period. When you move down a group, the number of valence electrons stay constant.(:
Wiki User
∙ 13y ago
Wiki User
∙ 14y agoIt increases. This is EXACTLY what the number groups mean! First row elements. It's on the left side. They have ONE valence electron.
Second row. 2 valence electrons.
Third row. 3 valence electrons.
All the way up to 8. The noble gases. Right hand side.
This kind of skews a bit when talking about transition metals but forget that for now. The D-Block isn't in your interests at this particular moment in time.
Sit down and give the Periodic Table a good stare. It's laid out like that for some very good reasons and this is one of them. It's trying to help you and make everything as simple as possible.
Wiki User
∙ 13y agoThe number of valence electrons stays the same as an investigator goes down the group on the periodic table. There is a good reason for this: the table was arranged that way. On purpose. An example might help.
In the Group 1 elements, we find lithium (Li), sodium, (Na), potassium (K) and on down the group. These are the alkali metals, and all of these elements have one electron in their valence shell.
The periodic table was arranged this way so that anyone who looks down a group could find elements with the same outer electron arrangements. This would make predicting their chemical behavior easier than if the elements were just on a list. And it works very well.
Wiki User
∙ 14y agono they decrease down any given group and increase across any given period.
Wiki User
∙ 11y agobecause the number of valence electrons goes up as you go down the periodic table since it adds a valence electrons
GAMEGRUMPS
Wiki User
∙ 11y agoI think to Left to Right :)
Anonymous
one minus one equals two.
Anonymous
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How many valence electrons does an atom have?
This all depends on the element's atomic number (number of protons). Since atoms have the same number of protons as they do electrons, the atomic number is essentially equal to the number of electrons as well. For example Aluminum atomic There are lists, but you can just tell anyway according to which group they are in. Eg, elements in the same column as Ca have 2 outer electrons (and a valency of +2), elements in the same column as Na have 1 outer electron (and a valency of +1). At the other end of the table, elements in the same column as Cl have 7 outer electrons, and a valency of -1 (8-7=1). work it out- you don't need a list.the number of electrons is equal to the atomic numberValence electrons are the electrons in the outer shell of the atom, just figure out which subshell is the outershell and then you will be able to work out the valence electrons.s shell holds 2p shell holds 6d shell holds 10f shell holds 14 See the Related Questions. Also, see the related links to download a .pdf version of a periodic table that lists the electron configuration for each element.
What is the trend of valence electrons across each period?
The number of valence electrons increases as you go across a period. For example in period 2 the number of valence electrons rises from 1 in Li up to 8 in neon.
What best explains the observed trend in atomic radii going down periodic table?
The more energy levels that are occupied by electrons, the larger the atomic radius.
Describe the trend in nonmetallic property of the elements in group 16?
The name of the group is the oxygen family. The valence number for elements in that group are -2. (gain or share two electrons) Oxygen, sulfur and selenium are nonmetals. Tellurium and Polonium are metalloids.
How would you relate the number of valence electron to their group number in the periodic table?
For main group chemistry, the trend followed would be as such, where "n" is the valence orbital: ns1 = group 1 ns2 = group 2 ns2 np1 = group 3 (also called group 13) ns2 np2 = group 4 (also called group 14) ns2 np3 = group 5 (also called group 15) ns2 np4 = group 6 (also called group 16) ns2 np5 = group 7 (also called group 17) ns2 np6 = group 8 (also called group 18) This rule can only be successfully applied to main group chemistry, the D and F blocks (transition metals, lanthanides and actinides) do not follow this.
Would the trend in atomic size cause an increase or a decrease in the attraction between the nucleus and the valence electron within the group as the atomic number increases?
Atomic size increases from top to bottom in a group due to increase in theshieldingeffect.As you go down the group shielding from core electrons increases (as more core electrons are added), therefore valence electrons experience weaker attraction forces from the nucleus and are located further away from it, resulting in an increase in size.If you move across a period the attraction between the nucleus and valence electrons increases because the number of protons and the number of valence electrons both go up whereas the number of core electrons stays the same (shielding decreases). In this case the size decreases.
How many valence electrons does an atom have?
This all depends on the element's atomic number (number of protons). Since atoms have the same number of protons as they do electrons, the atomic number is essentially equal to the number of electrons as well. For example Aluminum atomic There are lists, but you can just tell anyway according to which group they are in. Eg, elements in the same column as Ca have 2 outer electrons (and a valency of +2), elements in the same column as Na have 1 outer electron (and a valency of +1). At the other end of the table, elements in the same column as Cl have 7 outer electrons, and a valency of -1 (8-7=1). work it out- you don't need a list.the number of electrons is equal to the atomic numberValence electrons are the electrons in the outer shell of the atom, just figure out which subshell is the outershell and then you will be able to work out the valence electrons.s shell holds 2p shell holds 6d shell holds 10f shell holds 14 See the Related Questions. Also, see the related links to download a .pdf version of a periodic table that lists the electron configuration for each element.
What is the trend of valence electrons across each period?
The number of valence electrons increases as you go across a period. For example in period 2 the number of valence electrons rises from 1 in Li up to 8 in neon.
What is group trend in the first ionization energies?
Ionization energies decrease moving down a group, because the shielding effect reduces the pull of the nucleus on valence electrons. Making them easier to remove.
What best explains the observed trend in atomic radii going down periodic table?
The more energy levels that are occupied by electrons, the larger the atomic radius.
How many Valance electrons in oxygen?
6 Use the periodic table as a guide. As you go across from left to right the number of valence electrons increases. H = 1 Be = 2 B = 3 C = 4 N = 5 O = 6 F = 7 This trend stays the same all the way down each column. Usually periodic tables are marked on the top with roman numerals or something to signify how many valence electrons each element has.
Which trend decreases for metals down a group atomic radiusreactivity or melting point?
Melting points generally decrease as you go down a group for group I and group II metals. This does not apply to the transition metals. Reactivity of metals increases down a group due to a larger size and less effective charge between the nucleus and valence electrons. Atomic radius increases due to a higher principle number of electrons.
How many valence electrons does an atom?
An atom can have anywhere from 1 to 8 valence electrons. The number of valence electrons. Elements in the first column of the Periodic Table have one electron, those in the second have two. Those in the large block ins the middle (the transition elements, the lanthanides, and the actinides are generally considered to have two valence electron , though they have a property called variable valence. The trend of valence electrons continues in the block on the left side (the last six columns). The first column in this block has six valence electrons, and so forth until the last column in which the elements have eight valance electrons, except for helium which has two.
What trend is oberserved among the atomic radii of main-group elements down a group. eplain this trend?
The trend of atomic radius increases down a group on the periodic table. This occurs because each successive element down a group has another energy level. As more electrons are added, more energy levels are needed to hold the electrons.
Describe the trend in nonmetallic property of the elements in group 16?
The name of the group is the oxygen family. The valence number for elements in that group are -2. (gain or share two electrons) Oxygen, sulfur and selenium are nonmetals. Tellurium and Polonium are metalloids.
How would you relate the number of valence electron to their group number in the periodic table?
For main group chemistry, the trend followed would be as such, where "n" is the valence orbital: ns1 = group 1 ns2 = group 2 ns2 np1 = group 3 (also called group 13) ns2 np2 = group 4 (also called group 14) ns2 np3 = group 5 (also called group 15) ns2 np4 = group 6 (also called group 16) ns2 np5 = group 7 (also called group 17) ns2 np6 = group 8 (also called group 18) This rule can only be successfully applied to main group chemistry, the D and F blocks (transition metals, lanthanides and actinides) do not follow this.
Why ionization energy decreases from top to bottom in a group?
as atomic number is increase the size of the atom goes on increasing as more number of electron is added to the outer most orbit so the nuclear force exerted by the nucleus on electron is less so the affinity to loose electorn is more as the atomic number is increase that is the reason ionization energy decrease with increase in atomic number
