(a)
Interpretation:
The labeling of each atom in the polar covalent bond
Concept introduction:
Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. The more electronegative atom acquires a partial negative charge and the less electronegative atom acquires partial positive charge while showing charge distribution.
Answer to Problem 53E
The polar
Explanation of Solution
The electronegativity of an element increases along the period from left to right and decreases down in the group. From the figure
The polar
(b)
Interpretation:
The labeling of each atom in the polar covalent bond
Concept introduction:
Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. The more electronegative atom acquires a partial negative charge and the less electronegative atom acquires partial positive charge while showing charge distribution.
Answer to Problem 53E
The polar
Explanation of Solution
The electronegativity of an element increases along the period from left to right and decreases down in the group. From the figure
The polar
(c)
Interpretation:
The labeling of each atom in the polar covalent bond
Concept introduction:
Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. The more electronegative atom acquires a partial negative charge and the less electronegative atom acquires partial positive charge while showing charge distribution.
Answer to Problem 53E
The polar
Explanation of Solution
The electronegativity of an element increases along the period from left to right and decreases down in the group. From the figure
The polar
(d)
Interpretation:
The labeling of each atom in the polar covalent bond
Concept introduction:
Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. The more electronegative atom acquires a partial negative charge and the less electronegative atom acquires partial positive charge while showing charge distribution.
Answer to Problem 53E
The polar
Explanation of Solution
The electronegativity of an element increases along the period from left to right and decreases down in the group. From the figure
The polar
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Chapter 12 Solutions
Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
- Write an electron configuration for each element and the corresponding Lewis structure. Indicate which electrons in the electron configuration are included in the Lewis structure.(a) N(b) C(c) Cl(d) Ararrow_forwardTrue or False: The three most electronegative elements on the periodic table are fluorine, oxygen, and nitrogen.arrow_forward18.) Choose all the statements that are correct. (1) Like atomic size, electronegativity decreases going across a period and increases going down a group. (2) The second most electronegative element is chlorine. (3) Electronegativity is directly proportional to atomic number. (4) Like ionization energy, electronegativity increases going across a period and decreases going down a group. (5) Electronegativity is a measure of the ability of an atom to attract electrons and form a negative ion. (6) Electronegativity is a measure of the ability of an atom in a molecule to attract electrons go itself. (7) Electronegativity was first proposed by Linus Pauling. Group of answer choices (2) (1) (4) (3) (5) (7) (6)arrow_forward
- Compare the magnitude of the lattice energy for each of the following two ion pairs. (a) Ni²+ and O²- separated by a distance of 220 pm (b) Mn²+ and O²- separated by a distance of 431 pmarrow_forwardWrite Lewis dot symbols for the following atoms and ions: (a) I (b) I-(c) S(d) S2-(e) P (f) P3-(g) Na (h) Na+(i) Mg (j) Mg2+arrow_forwardDraw Lewis diagrams for the following ions. In the formula the symbol of the central atom is given first. (Hint:The valence octet may be expanded for the central atom.)(a) BrO4 - (b) PCl6 - (c) XeF6+arrow_forward
- Show how each chemical change obeys the octet rule. (a) Hydrogen forms H2 (hydride ion)arrow_forwardMany monatomic ions are found in seawater, including the ions formed from the following list of elements. Write the Lewis symbols for the monatomic ions formed from the following elements:(a) Cl(b) Na(c) Mg(d) Ca(e) K(f) Br(g) Sr(h) Farrow_forwardWhat is the molecular geometry (shape) of the ammonium chloride molecule?arrow_forward
- 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-Harrow_forward3) The molecule diphosphorus tetraoxide (P,O,) has two central atoms and four different resonance structures that do not violate the octet rule. Draw two of these resonance structures below. 4) The compound acetone is a common solvent. It has a chemical formula of CH,COCH, Acetone has three central atoms. (a) Draw the Lewis Dot structure for acetone. (b) Give the Ideal Bond Angle for all three central atoms. 5) Four covalent molecules are drawn below. :o: H. H-CH H H (1) (2) (3) (4) a) Define each of these molecules as polar or non-polar. (1) (2) (3) b) Describe the type of intermolecular force that each molecule would use: (1) (2) (3) (4)arrow_forwardFrom its position in the periodic table, determine which atom in each pair is more electronegative:(a) Br or Cl(b) N or O(c) S or O(d) P or S(e) Si or N(f) Ba or P(g) N or Karrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_forward_ios
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning