Number Of Valence Electrons In Magnesium

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Valence Electrons

  1. Number Of Valence Electrons In A Magnesium Atom
  2. Amount Of Valence Electrons In Magnesium

Valence Electrons and Ion Formation for the First 20 Elements Element Total Number of Electrons in Neutral Atom Valence Electrons Gain or Lose Electrons Ion Formed Hydrogen 1 1 Gain or Lose 1 H+ or H-Helium 2 2 None None Lithium 3 1 Lose 1 Li+ Beryllium 4 2 Lose 2 Be2+ Boron 5 3 Lose 3 B3+.

Chemistry is a study of different atoms, an atom is the smallest particle in matter. An atom consists of three major subatomic particles, which are electrons, neutrons and protons. The protons are the positively charged particles. The neutrons are the neutral particles. The electrons are the negatively charged particles. The neutrons and protons are located inside the nucleus of the atom. An atom has nucleus in the center, around the nucleus are electrons arranged in various orbits depending on the atomic number.

Valence electrons definition:

Every atom has a unique atomic number. The number of electrons an atom has is equal to the atomic number of the atom. Initially the atom fills electrons in the inner most orbit and then the outer orbits. Theses electrons are arranged in orbits around the nucleus. The electrons that are present in the outermost shell of the atom are called as the valence electrons. Identifying the number of valence electrons for each atom is a very useful concept which can be applied in chemical bonding and many other chemistry topics.
The following is a table to understand the number of valence electrons the atoms in the periodic table have:
  1. The number of electrons in each element’s electron shells, particularly the outermost valence shell, is the primary factor in determining its chemical bonding behavior. In the periodic table, the elements are listed in order of increasing atomic number Z. Electron configuration of Magnesium is Ne 3s2. Possible oxidation states are +2.
  2. - 13897653 Xenon has eight valence electrons, which are the electrons in its outer shell. Magnesium is element 12 and belongs to Group 2 of the Periodic Table. Zinc has 2, 8, 18, 2, so it has 2 valence electrons. The number of valence electrons is determined by how many electrons are in the last energy level (the one furthest from the.
  3. Since the 3s² electrons are the outermost electrons, magnesium has two valence electrons.
  4. Magnesium has 2 valence electrons. For the main group elements (not transition metals), the group number tells us the number of valence electrons in. See full answer below. Become a member.
Periodic Table Group Number of valence electrons
The Alkali metals (Group I) 1
The Alkaline earth metals (Group II) 2
The transition metals (Group 3 to 12) 3-12
Group III 3
Group IV 4
Group V 5
Group VI 6
The Halogens 7
Noble Gases Group (VIII) 8

Writing Electronic Configuration for finding the valence electrons:

The electronic configuration of an atom can be written according its atomic number. The number of electrons of an atom are arranged in sub energy levels at the ground state of the atoms. The electronic configuration of an atom starts by filling the lower sub energy levels. Given below is the chart that helps to identify how the electrons are filled and the order in which the electronic configuration is written:
So the order in which the electrons are filling is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s and so on.
Valence electrons of few atoms:
The following are examples of finding the number of valence shell electrons using the electronic configuration of the given atom.
Valence electrons of Hydrogen:
· The atomic number of Hydrogen is 1.
· The electronic configuration for Hydrogen is 1s1.
· The number of valence electrons is 1. Since the 1s shell is the outermost shell it has only one electron in it. The orbits for the Hydrogen atom looks like this:
Valence electrons of Helium:
· The atomic number of Helium is 2.
· The electronic configuration for Helium He is 1s2.
· The number of valence electrons is 2. The number of electrons it has is 2.
The diagram for the Helium atom looks like this:
Valence electrons of Lithium:
· The atomic number of Lithium is 3.
· The electronic configuration for Lithium Li is 1s2, 2s1.
· The outermost shell of Lithium is 2s. The number of valence electrons is has 1.
The diagram for the Helium atom looks like this:
Valence electrons of Beryllium:
· The atomic number of Beryllium is 4.
· The electronic configuration for Beryllium Be is 1s2, 2s2.

Number Of Valence Electrons In A Magnesium Atom


· The outermost shell of Beryllium is 2s. The number of valence electrons is has 2. The diagram for the Beryllium atom looks like this:
Valence electrons of Boron:
· The atomic number of Boron is 5.
· The electronic configuration for Boron B is 1s2, 2s2, 2p1.
· The outermost shell of Boron is n = 2. The total number of valence electrons it has is 3. The diagram for the Boron atom looks like this:
Valence electrons of Carbon:
· The atomic number of Carbon is 6.
· The electronic configuration for Carbon C is 1s2, 2s2, 2p2.
· The outermost shell of Carbon is n = 2. The total number of valence electrons it has is 4. The diagram for the Carbon atom looks like this:
Valence electrons of Nitrogen:
· The atomic number of Nitrogen is 7.
· The electronic configuration for Nitrogen is N 1s2, 2s2, 2p3.
· The outermost shell of Nitrogen N is n = 2. The total number of valence electrons it has is 5. The diagram for the Nitrogen atom looks like this:
Valence electrons of Oxygen:
· The atomic number of Oxygen is 8.
· The electronic configuration for Oxygen O is 1s2, 2s2, 2p4.
· The outermost shell of Oxygen is n = 2. The total number of valence electrons it has is 6. The diagram for the Oxygen atom looks like this:
Valence electrons of Fluorine:
· The atomic number of Fluorine is 9.
· The electronic configuration for Fluorine F is 1s2, 2s2, 2p5.

Amount Of Valence Electrons In Magnesium


· The outermost shell of Fluorine is n = 2. The total number of valence electrons it has is 7. The diagram for the Fluorine atom looks like this:
Valence electrons of Neon:Number Of Valence Electrons In Magnesium
· The atomic number of Neon is 10.
· The electronic configuration for Neon Ne is 1s2, 2s2, 2p6.
· The outermost shell of Neon is n = 2. The total number of valence electrons it has is 8. The orbits of Neon atom looks like this:
Valence electrons of Sodium:
· The atomic number of Sodium is 11.
· The electronic configuration for Sodium Na is 1s2, 2s2, 2p6, 3s1.
· The outermost shell of Sodium Na is n = 3. The total number of valence electrons it has is 1. The orbits of Sodium atom looks like this:
Valence electrons of Magnesium:
· The atomic number of Magnesium is 12.
· The electronic configuration for Magnesium Mg is 1s2, 2s2, 2p6, 3s2.
· The outermost shell of Magnesium Mg is n = 3. The total number of valence electrons it has is 2. The orbits of Magnesium atom looks like this:
Valence electrons of Aluminum:
· The atomic number of Aluminum is 13.
· The electronic configuration for Aluminum Al is 1s2, 2s2, 2p6, 3s2, 3p1.
· The outermost shell of Aluminum Al is n = 3. The total number of valence electrons it has is 3. The orbits of Aluminum atom looks like this:
Shown above are the valence electrons for atoms with atomic number 1 to 13. The same concept applies for finding the valence electrons of all the atoms in the periodic table.

Valence Electrons and Octets

The number of valence electrons, those electrons in the outermost energy level, determines the number of electrons an element will gain or lose. Since the families have the same pattern of outer electrons, the number of valence electrons is the same in each family.

The table above is a result of atoms losing and gaining electrons to form stable noble gas electron configurations. When an element loses electrons it commonly does so until all valence electrons are gone; thus, magnesium with 2 valence electrons will react to become Mg2+, magnesium cation by losing the 2 valence electrons. Likewise, when an element gains electrons, it will gain only enough electrons to fill the outer shell s and p-orbitals; such as, nitrogen with 5 valence electrons will gain 3 electrons to become N3–, nitrogen anion, so that there are 8 electrons in the outer shell. The full outer shell of 8 electrons is is called an octet, and ions are said to be stable when they have an octet. Here are two more examples:

  • K = [Ne]3s1 ➔ (lose 1e – ) ➔ [Ne] = 1s22s22p6 = K1+
  • S = [Ne]3s23p4 ➔ (gain 2e – ) ➔ [Ne]3s23p6 = S2– .

Noble gases do not react because they already have full shells, ns2np6. The energy change when electrons are added or removed is too large because the effective nuclear charge is too high for an electron to be removed easily and because adding electrons would require using a new shell which is not favorable. For nonmetals in the second period that lose electrons, the number of electrons lost will result in the noble gas electron configuration of helium 1s2, so only two valence electrons are in the outer shell not an octet. Hydrogen usually loses one electron to become a single proton in the nucleus without any electrons in the electron cloud, H+; however, it very occasionally gains one electron to become H– with an electron configuration similar to helium.