Concept explainers
(a)
Interpretation:
Resonance structures of
Concept Introduction:
Resonance structures refers to different forms of a same molecule which has same
(b)
Interpretation:
Resonance structures of
Concept Introduction:
Resonance structures refers to different forms of a same molecule which has same chemical bonding between the atoms but different electron distribution among the atoms in the molecule.
(c)
Interpretation:
Resonance structures of
Concept Introduction:
Resonance structures refers to different forms of a same molecule which has same chemical bonding between the atoms but different electron distribution among the atoms in the molecule.
(d)
Interpretation:
Electron dot structure of
Concept Introduction:
Electron dot structure also known as Lewis dot structure is a diagram representing a compound revealing the valence electrons of the constituent atoms.
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General Chemistry: Atoms First
- (1) What is the total number of valence electrons in the Lewis structure of SF2? electrons (2) Draw a Lewis structure for SF2arrow_forwardshorter than the O-O bond in O2? Explain. 8.37 Which of the following statements about electronegativity is false? (a) Electronegativity is the ability of an atom in a molecule to attract electron density toward itself. (b) Electronegativity is the same thing as electron affinity. (c) The numerical values for electronegativity have no units. (d) Fluorine is the most electronegative element. (e) Cesium is the least electronegative element. 8,38 (a) What is the trend in electronegativity going fromarrow_forwardWrite the Lewis structure for each molecule. These molecules do not follow the octet rule.(a) BCl3(b) NO2(c) BH3arrow_forward
- Draw all possible resonance structures for each of these compounds. Determine the formal charge on each atom in each of the resonance structures:(a) O3(b) SO2(c) NO2 −(d) NO3−arrow_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_forwardThese species do not obey the octet rule. Draw a Lewis structure for each, and state the type of octet-rule exception:(a) PF₆(b) ClO₃(c) H₃PO₃(one P−H bond)arrow_forward
- Calculate the enthalpy change for the following reactions using the bond enthalpy given below. (Bond enthalpy/kJ : H−H = 436, C−H = 413, C=O = 799, O=O = 495, O−H = 463) (a) H2(g) + 1⁄2O2(g) → H2O(g) (b) CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)arrow_forwardIodine forms a series of fluorides (listed here). Write Lewis structures for each of the four compounds and determine the formal charge of the iodine atom in each molecule:(a) IF(b) IF3(c) IF5(d) IF7arrow_forwardDraw Lewis structures for HFO4, HFO3, HC0O4, HC0O3, HCO2. (These molecules have the halogen atom as the central atom. All O atoms are attached to the halogen. The hydrogen atom is bonded to one of the O atoms.) Use formal charges to determine which molecule is least likely to occur in nature. (A) HFO4 (B) HC(O2 (C) HC!O3 (D) HFO3 (E) HC\O4 DO000arrow_forward
- Write Lewis structures for the following molecules or ions. (Assign lone pairs, radical electrons, and atomic charges where appropriate.) (a) BrF3 (b) AsF5 (c) BI3 (d) AsF6−arrow_forwardDraw Lewis structures for each of the following compounds. In each case, specify the number of valence electrons surrounding the central atom. (Assign lone pairs and radical electrons where appropriate.) (Assume the central atom does not contain an expanded octet.) (a) bromine dioxide (BrO2) (b) beryllium bromide (BeBr2) (c) phosphorus pentafluoride (PF5)arrow_forwardWrite Lewis dot symbols for the following atoms and ions. (a) I (b) I− (c) S (d) S2−arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning