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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.
Yazmin Sawayn
Wiki User
∙ 15y agothe number of electrons changes with the number of protons, and the number of protons = the atomic # (represented with "Z"). The numbers increase by 1 each step to the right, then continues each row down.
i.e. Hydrogen has 1 electron, Helium has 2, Lithium then has 3, etc.
however, the number of valence (outermost shell) electrons resets every row
i.e. Hydrogen has 1 valence electron, Helium has 2, then Lithium has 1
if this did not help, I suggest you go to http://webelements.com/ (an online Periodic Table)
Wiki User
∙ 13y agoAcross a period, from left to right, atomic number (no. of protons) increases consecutively. The no. of protons is equal to the no. of electrons in an element.
Therefore, Across a period, from left to right, no. of electrons increases consecutively.
Wiki User
∙ 11y agoThe number of valence electrons generally increase from left to right across the periodic table. The elements in group 1 have one valence electron. The elements in group 18 have eight valence electrons.
Wiki User
∙ 11y agothey get more electrons the farther right the get
Wiki User
∙ 11y agoThe 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.
Wiki User
∙ 16y agothey increase
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What is the trend for ionic radius for medals?
if you mean metals ..... for the same valence the radius decreases across a period and increases down a family
What trend electronegativity do you see across period on the periodic table?
The trend as you move from left to right across a period in the periodic table, the electronegativity increases due to the stronger attraction that the atoms obtain as the nuclear charge increases. Moving down a group, the electronegativity decreases due to the longer distance between the nucleus and the valence electron shell, thereby decreasing the attraction, making the atom have less of an attraction for electrons or protons.
What is is the trend across a period?
what is the reason for ionization energy across a period
What factors need to be considered when predicting the trend in ionisation energies across a period?
The charge on the nucleus.The distance of the electron from the nucleus.The number of electrons between the outer electrons and the nucleus.
Is the trend across a period similar or different for periods 2 3 4 and 5?
Similar for they have the same number of electrons in the last shell
What is the trend for ionic radius for medals?
if you mean metals ..... for the same valence the radius decreases across a period and increases down a family
In general - what happens to the atomic radius from left to right across a period?
Generally, it decreases.*As you move from left to right across a period the elements' number of protons increases, increasing the effective nuclear charge (the charge felt by the outermost [valence] electrons after taking into account the shielding electrons). As effective nuclear charge increases the attraction between the nucleus and the valence electrons increases, pulling the valence electrons closer to the nucleus, decreasing the atomic radius.*Please understand that this is not a hard and fast rule. There are other factors to take into account when determining atomic radius, this is just a general trend witnessed.
What trend electronegativity do you see across period on the periodic table?
The trend as you move from left to right across a period in the periodic table, the electronegativity increases due to the stronger attraction that the atoms obtain as the nuclear charge increases. Moving down a group, the electronegativity decreases due to the longer distance between the nucleus and the valence electron shell, thereby decreasing the attraction, making the atom have less of an attraction for electrons or protons.
What is is the trend across a period?
what is the reason for ionization energy across a period
What factors need to be considered when predicting the trend in ionisation energies across a period?
The charge on the nucleus.The distance of the electron from the nucleus.The number of electrons between the outer electrons and the nucleus.
Is a trend across a period similar or different for periods 2 3 4 and 5?
Similar for they have the same number of electrons in the last shell
Is the trend across a period similar or different for periods 2 3 4 and 5?
Similar for they have the same number of electrons in the last shell
What is the trend in electronegativity and ionization energy as you go down a row or across a period?
Electron configuration is the arrangement of elements according to their increasing atomic numbers whiles period is the arrangement of elements according to the increasing number of valence electrons.
Why does the general electronegativity trend increases across the same period?
The general electronegativity trend increases across the same period due to the increasing effective nuclear charge, which attracts the electrons more strongly towards the nucleus. As you move from left to right across a period, the number of protons in the nucleus increases while the shielding effect remains relatively constant, resulting in a greater attraction for electrons and higher electronegativity values.
What is the periodic trend for ionization energy and electron affinity?
Ionization energy increases from left to right across a period, and decreases down a group.
Why does the trend in electronegativey of elements across a period increase from left to right?
It increases from left to right across a period because as electrons are added to the same energy level, and the closer an atom gets to having an octet of electrons, the easier it is for the atom to attract electrons from other atoms, either through ionic bonding or covalent bonding.
What is the trend for electrons?
As you go across a period; Left to right, the electron affinity increases. As you go down a group; top to bottom, the electron affinity decreases.
