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a.
To determine:
The Lewis structure of
Introduction:
The Lewis structures are also called electron dot structures. In the Lewis structure, electrons are denoted by dots. These dots represent the number of electrons present in the outer most shell of an element.
To determine:
The labeled polar covalent bond of
Introduction:
The dipole moment in the molecule arises due to the electronegativity difference between the atoms. The dipole moment of the symmetric molecule is zero because the electron withdrawing molecules cancel each other’s dipole moments. However, the dipole moment of unsymmetrical molecules is not zero. There is always a net dipole moment.
To determine:
The molecule is polar or non-polar and the dipole moment arrow of the molecule.
Introduction:
The polarity of a bond is directly related to the electronegativity difference. A polar bond corresponds to a non-uniform distribution of the electron cloud between two nonmetals. Thus, the bond formed between them is a covalent bond. This corresponds to the fact that an atom with higher electronegativity value will show a higher affinity for electrons.
A non-polar bond is formed by a mononuclear diatomic molecule that corresponds to a uniform distribution of the electron cloud. These molecules do not possess a dipole moment.
b.
To determine:
The Lewis structure of
Introduction:
The Lewis structures are also called electron dot structures. In the Lewis structure, electrons are denoted by dots. These dots represent the number of electrons present in the outer most shell of an element.
To determine:
The labeled polar covalent bond of
Introduction:
The dipole moment in the molecule arises due to the electronegativity difference between the atoms. The dipole moment of the symmetric molecule is zero because the electron withdrawing molecules cancel out each other’s dipole moments. However, the dipole moment of unsymmetrical molecules is not zero. There is always a net dipole moment.
To determine:
The molecule is polar or non-polar and the dipole moment arrow of the molecule.
Introduction:
The polarity of a bond is directly related to the electronegativity difference. A polar bond corresponds to a non-uniform distribution of the electron cloud between two nonmetals. Thus, the bond formed between them is a covalent bond. This corresponds to the fact that an atom with higher electronegativity value will show a higher affinity for electrons.
A non-polar bond is formed by a mononuclear diatomic molecule that corresponds to a uniform distribution of the electron cloud. These molecules do not possess a dipole moment.
c.
To determine:
The Lewis structure of
Introduction:
The Lewis structures are also called electron dot structures. In the Lewis structure, electrons are denoted by dots. These dots represent the number of electrons present in the outer most shell of an element.
To determine:
The labeled polar covalent bond of
Introduction:
The dipole moment in the molecule arises due to the electronegativity difference between the atoms. The dipole moment of the symmetric molecule is zero because the electron withdrawing molecules cancel out each other’s dipole moments. However, the dipole moment of unsymmetrical molecules is not zero. There is always a net dipole moment.
To determine:
If the molecule is polar or non-polar and the dipole moment arrow of the molecule.
Introduction:
The polarity of a bond is directly related to the electronegativity difference. A polar bond corresponds to a non-uniform distribution of the electron cloud between two nonmetals. Thus, the bond formed between them is a covalent bond. This corresponds to the fact that an atom with higher electronegativity value will show a higher affinity for electrons.
A non-polar bond is formed by a mononuclear diatomic molecule that corresponds to a uniform distribution of the electron cloud. These molecules do not possess a dipole moment.
d.
To determine:
The Lewis structure of
Introduction:
The Lewis structures are also called electron dot structures. In the Lewis structure, electrons are denoted by dots. These dots represent the number of electrons present in the outer most shell of an element.
To determine:
The labeled polar covalent bond of
Introduction:
The dipole moment in the molecule arises due to the electronegativity difference between the atoms. The dipole moment of the symmetric molecule is zero because the electron withdrawing molecules cancel out each other’s dipole moments. However, the dipole moment of unsymmetrical molecules is not zero. There is always a net dipole moment.
To determine:
The molecule is polar or non-polar and the dipole moment arrow of the molecule.
Introduction:
The polarity of a bond is directly related to the electronegativity difference. A polar bond corresponds to a non-uniform distribution of the electron cloud between two nonmetals. Thus, the bond formed between them is a covalent bond. This corresponds to the fact that an atom with higher electronegativity value will show a higher affinity for electrons.
A non-polar bond is formed by a mononuclear diatomic molecule that corresponds to a uniform distribution of the electron cloud. These molecules do not possess a dipole moment.
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Chapter 3 Solutions
General, Organic, and Biological Chemistry (3rd Edition)
- Classify each compound as ionic or molecular: a.COb.ZnBr2c.CH4d.NaFarrow_forward5. Fill in the empty boxes with the correct information. 6. 1st Element Ag # of atoms 1 b. Ionic bond: 2nd Element c. Polyatomic Ion NO₂ # of atoms Give three chemical formulas and corresponding names for each bonding pattern: a. Covalent bond: 81 Formula C8H10 Name Ammonium phosphate Molybdenum (II) acetate Potassium telluratearrow_forwardIonic compounds do not consist of molecules, but covalent compounds generally do. Why is it incorrect to refer to a molecule of an ionic compound? As part of your answer, draw two scenes, representing atoms as circles: a. Draw at least 6 copies of NaCl showing how it is bonded. b. Draw at least 6 copies of BrCl showing how it is bonded. Then explain what is meant by a molecule and why it is correct to state that most covalent compounds exist as molecules, but ionic compounds do not exist as molecules. Take a picture of your drawing and explanation and insert it in the answer box.arrow_forward
- Pls help me answer these questions properly. Thanks. 1. Write the general rule for determining whether a chemical formula represents an ionic or a covalent compound. 2. Which of the following formulas describe ionic and/or covalent compounds? a. NaCl b. CO2 c. CaCl2 d. HCl e. CH3Br f. BeCl2 g. NH4NO3 h. Ba(NO3)2arrow_forward1. All of the following are used in writing Lewis dot symbols EXCEPT what? a. element symbolb. mass numberc. number of valence electronsd. group number in the periodic table 2. Which is the formula of the compound formed by barium and phosphorus? a. Ba3 Pb. Ba2 Pc. BaP3d. Ba3 P2arrow_forwardWrite the formula for each molecule.a. chlorine monoxideb. arsenic acidc. phosphorus pentachlorided. hydrosulfuric acidarrow_forward
- 12. In number 11, the subscript 2 represents what? a. The charge on OH b. The negative charge from copper. c. The positive charge from copper. d. How many copper atoms it took to fulfill the octet of hydroxide. 13. Name the following compound, CuCl2. a. Copper dichloride b. Copper (II) chlorine c. Monocopper dichloride d. Copper (II) chloride 14. Name the compound CoBr2. a. Copper dibromide b. Cobalt dibromide c. Cobalt (II) bromide d. Cobalt bromide 15. What is the chemical formula for calcium phosphate? a. Ca3P2 b. Ca3(PO4)2 c. CaPO4 d. Ca2(PO4)3 16. Which of the following substances have the weakest intermolecular force? a. A substance whose boiling point is 85 degrees. b. A substance that evaporates at 30 degrees. c. Ice d. Room-temperature corn syrup 17. The difference between intermolecular forces and intramolecular forces is that a. Intramolecular forces require more energy to break than intermolecular forces b. Intermolecular forces are bonds and intramolecular forces are…arrow_forwardDraw the lewis diagram for Cl2 and answer the following question: (Please show your work when drawing the lewis diagram) a. How many LONE PAIRS of electrons are in the chlorine molecule, Cl2? b. How many BONDING PAIRS of electrons are there in this molecule? c. What type of bond (ionic or covalent) exists between these two atoms? (CI2 as two chlorine atoms bonded together, NOT a carbon and two iodine atoms. CI2 is a diatomic Chlorine molecule!)arrow_forwardQuestion 4,5,6,7arrow_forward
- 68. Classify each of the following compounds as either (1) a binary ionic compound, (2) an ionic compound with polyatomic ion(s), (3) a binary covalent compound, (4) a binary acid, or (5) an oxyacid. Write the chemical formula that corresponds to each name. a. potassium sulfide b. sulfuric acid c. ammonium nitrate d. iodine pentafluoride e. copper(I) sulfate f. hydrofluoric acid g. sodium hydrogen carbonatearrow_forward12. Which of the following is NOT an ionic compound? a. K2O b. NaCl c. NazSO4 d. CO2 e. LIN3arrow_forward6. Draw a picture of each of the following. a. an ionic crystal lattice c. a molecular compound b. a diatomic element d. a mixture of nitrogen gas and water vapor How do your drawings illustrate the difference between compounds and mixture? How do your drawings illustrate the difference between ionic and molecular compounds?arrow_forward
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