How many bonds can each atom make without hybridization? B,N, and O

B is 3

N is 3
O is 2

To determine how many bonds each atom can make without hybridization, we need to consider the number of valence electrons each atom possesses. Valence electrons are the electrons found in the outermost energy level of an atom and are involved in bonding.

1. Boron (B):
Boron is located in Group 3 of the periodic table and has an atomic number of 5. It has 3 valence electrons in its outermost energy level (2s^2 2p^1). Without hybridization, boron can make a maximum of 3 bonds (one for each valence electron).

2. Nitrogen (N):
Nitrogen is located in Group 15 of the periodic table and has an atomic number of 7. It has 5 valence electrons in its outermost energy level (2s^2 2p^3). Without hybridization, nitrogen can make a maximum of 3 bonds as well. This is because one of its p-orbitals can only hold a maximum of 2 electrons, leaving one unpaired electron to form a bond.

3. Oxygen (O):
Oxygen is located in Group 16 of the periodic table and has an atomic number of 8. It has 6 valence electrons in its outermost energy level (2s^2 2p^4). Without hybridization, oxygen can make a maximum of 2 bonds. Just like nitrogen, oxygen's p-orbitals can only hold a maximum of 2 electrons, resulting in two unpaired electrons available for bonding.

Keep in mind that although these elements can form a certain number of bonds without hybridization, they can undergo hybridization to form additional bonds by rearranging their valence electrons. Hybridization allows atoms to form bonds using orbitals that are mixtures of different atomic orbitals.