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Answer: Option (B) is the correct answer.
Explanation:
Isotopes are the substances or species that contain same number of protons but different number of neutrons.
As it is known that atomic number means the total number of protons present in an atom. Hence, this also means that in isotopes atomic number of the species is same.
For example, isotopes of hydrogen are ,
, and
.
Isotopes of only heavier elements are radioactive in nature as they have large difference in the number of protons and neutrons.
Thus, we can conclude that the statement isotopes of the same element have the same atomic number but differ in their atomic masses, is correct.
Answer:
The required hybridization for a central atom that have:
a tetrahedral arrangement of electron pairs is
a trigonal planar arrangement of electron pairs is
a linear arrangement of electron pairs is
Explanation:
From the given information:
The required hybridization for a central atom that have:
a tetrahedral arrangement of electron pairs is
a trigonal planar arrangement of electron pairs is
a linear arrangement of electron pairs is
Hybridization is the mixing and blending of two or more pure atomic orbitals ( s, p and d) to forma two or more hybrid atomic orbitals that are identical in shape and energy e. sp ,sp² , sp³, sp³d hybrid orbitals.
Examples:
Tetrahedral
In CH₄ , carbon C is the central atom.
A 2s electron is excited from the ground state of boron 1s²2s²2p² to one of the empty orbitals to 2p to give the excited state 1s²2s²2p³.
In the excited state of carbon, the 2-s orbital can be mixed with the 2p orbitals in three ways : sp³, sp² and sp hybridization. For the formation of four sp³ hybrid orbitals, the 2s orbital are mixed with all the three p orbitals. The four sp³ hybrid orbitals are tetrahedrally arranged with a bond angle of 109.5⁰
Trigonal Planar
In BF₃ , Boron B is the central atom
A 2s electron is excited from the ground state of boron 1s²2s²2p¹ to one of the empty orbitals to 2p. The 2s orbital is then mixed with two orbitals of 2p to form three sp² hybrid orbitals that are trigonal planar arranged in the plane in order to minimize repulsion. They bonds between them form an equal strength and with bond angles of 120⁰
Linear arrangement:
In BeCl₂, Be is the central atom
To provide the unpaired electrons for covalent bonds a 2s electron is excited to a 2p orbital. Thereafter, the two atomic orbitals hybridize to give two identical orbitals called sp hybrid orbitals. The sigma bond for,ed are equal in bond lengths and form a bond angle of 180°