(a) Interpretation: A formula for an ionic compound should be given using only P, Br and Mg. Concept introduction: Ionic bonds form due to the complete loss or gain of one or more electrons resulting in cations and anions. They are held together by electrostatic interactions. In most cases, bonds form between two atoms are not completely ionic but have some covalent character. The magnitude of covalent character and ionic character is determined by the difference between electronegativity of the two atoms. Higher the difference, higher the ionic character.
(a) Interpretation: A formula for an ionic compound should be given using only P, Br and Mg. Concept introduction: Ionic bonds form due to the complete loss or gain of one or more electrons resulting in cations and anions. They are held together by electrostatic interactions. In most cases, bonds form between two atoms are not completely ionic but have some covalent character. The magnitude of covalent character and ionic character is determined by the difference between electronegativity of the two atoms. Higher the difference, higher the ionic character.
Solution Summary: The author explains that ionic bonds form due to the complete loss or gain of one or more electrons resulting in cations and anions.
A formula for an ionic compound should be given using only P, Br and Mg.
Concept introduction:
Ionic bonds form due to the complete loss or gain of one or more electrons resulting in cations and anions. They are held together by electrostatic interactions. In most cases, bonds form between two atoms are not completely ionic but have some covalent character. The magnitude of covalent character and ionic character is determined by the difference between electronegativity of the two atoms. Higher the difference, higher the ionic character.
Interpretation Introduction
(b)
Interpretation:
The formula of the molecular compound having polar covalent bonds needs to be determined. The molecular compound obeys the octet rule and there is no formal charge on it.
Concept introduction:
When an atom has a different number of electrons than the number of valence electrons, then the atom has either gained or removed electrons. So, that particular atom bears a formal charge. The formal charge can be calculated by following formula.
Formal charge = No. of valence electrons - 12 No. of bonding electrons - No. of nonbonding electrons
Which of the following compounds has both ionic and covalent bond?
(a) H2O
(b) NH4Cl
(c) NaCl
(d) HCl
Which statements are true about electronegativity?
(a) Electronegativity increases from left to right in a period of the Periodic Table.
(b) Electronegativity increases from top to bottom in a column of the Periodic Table
. (c) Hydrogen, the element with the lowest atomic number, has the smallest electronegativity.
(d) The higher the atomic number of an element, the greater its electronegativity.
ii.
Answer true or false.
(a) A covalent bond is formed between two atoms whose difference in electronegativity is less
than 1.9.
(b) If the difference in electronegativity between two atoms is zero (they have identical
electronegativities), then the two atoms will not form a covalent bond.
(c) A covalent bond formed by sharing two electrons is called a double bond.
(d) In the hydrogen molecule (H2), the shared pair of electrons completes the valence shell of
each hydrogen.
(e) In the molecule CH4, each hydrogen has an electron configuration like that of helium, and
carbon has an electron configuration like that of neon.
(f) In a polar covalent bond, the more electronegative atom has a partial negative charge (8-)
and the less electronegative atom has a partial positive charge (&+).
(g) These bonds are arranged in order of increasing polarity C-H