The carbon atom belongs to the second period of. The outermost and highest energy level is 4, containing two valence electrons (4s 2). We know that the atomic number of carbon is 6.Therefore there will be 6 electrons present in its o-orbitals. The number of notations in the electronic configuration will show the number of. The Atomic Number(Z) of Calcium (Ca) is 20, and the electronic configuration of Ca is 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2. Carbon has 6 electrons, 2 in the 1st shell and 4 in the 2nd shell. The ten core electrons are in shells 1 and 2 (1s 2 2s 2 2p 6). The outermost shell is 3 with two valence electrons (3s 2). The Atomic Number(Z) of Magnesium (Mg) is 12, and the electronic configuration is 1s 2 2s 2 2p 6 3s 2. Both have the same number of two valence electrons. Magnesium and Calcium belong to Group number 2.

The outermost shell is 3 with 6 valence electrons (3s 2 3p 4). The electronic configuration of S is 1s 2 2s 2 2p 6 3s 2 3p 4. The Atomic Number(Z) of Sulfur (S) is 16 with 16 electrons. The two core electrons are present in shell 1 (1s 2). The farthest shell from the nucleus is 2 with six valence electrons (2s 2 2p 4). The electronic configuration of O is 1s 2 2s 2 2p 4. The Atomic Number(Z) of Oxygen (O) is 8, corelating to 8 electrons. Oxygen and Sulfur belong to the same group 16 in the periodic table and therefore have the same number of 6 valence electrons. The outermost shell is 3, containing five valence electrons (3s 2 3p 3), and the core electrons are in the inner 1 and 2 shells (1s 2 2s 2 2p 6). The electronic configuration of P is 1s 2 2s 2 2p 6 3s 2 3p 3. The Atomic Number (Z) of Phosphorus (N) is 15, with 15 electrons distributed into various shells and orbitals. So, the outermost shell is 2, containing five valence electrons.

The Atomic Number (Z) of Nitrogen (N) is 7, and its electronic configuration is 1s 2 2s 2 2p 3. The valence electrons of both Nitrogen and Phosphorus are 5.

The elements belonging to the same group have the same valence electrons. These bonds store an enormous amount of energy. The outermost shell 3 contains four valence electrons (3s 2 3p 2), and the remaining are Silicon's core electrons in shells 1 and 2 (1s 2 2s 2 2p 6).Ĭarbon and Silicon belong to the same group 15 in the periodic table. Carbon's electron configuration of allows it to form very stable bonds with oxygen and hydrogen. Its electronic configuration is 1s 2 2s 2 2p 6 3s 2 3p 2. The outermost shell is 2, containing four valence electrons (2s 2 2p 2), and the two core electrons are in shell 1 (1s 2). Its electronic configuration after dividing the electrons into shells and orbitals is - 1s 2 2s 2 2p 2. So, both Carbon and Silicon will have four valence electrons. The only difference will be their shell number due to the increase in atomic size. All elements belonging to the same group in the periodic table will have the same number of valence electrons (table A). The group number and atomic number is used to determine the valence electrons of an element.Ĭarbon and Silicon belong to the same group 14 in the periodic table.

Carbon electron configuration number