Concept explainers
Interpretation:
The complete Lewis structures of the given compound have to be drawn. The different molecular geometries around each atom have to be identified. The atoms possessing tetrahedral geometry has to be rounded by circles, trigonal planar geometry has to be indicated by squares, trigonal pyramid geometry has to be denoted by pentagon, bent geometry has to be indicated by hexagon and atoms having unexpected number of bonds has to be indicated by triangle.
Concept Introduction:
Lewis structure:
The representation of valence shell electrons around the atom is known as Lewis structure or Lewis dot structure. Electrons are represented as a dot in Lewis structures, a single dot represents unpaired electron and paired of dots represents paired electrons.
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EBK FOUNDATIONS OF COLLEGE CHEMISTRY
- Draw Lewis structures to illustrate the bonding in the following molecules. In each case, there will be at least one multiple bond present in a molecule. a. COCl2: Both chlorine atoms and the oxygen atom are bonded to the carbon atom. b. C2H2Br2: The two carbon atoms are bonded to one another. Each carbon atom also has a bromine atom and a hydrogen atom bonded to it. c. C2N2: The two carbon atoms are bonded to one another, and each carbon atom also has a nitrogen bonded to it. d. CH2N2: A central carbon atom has both nitrogen atoms bonded to it. Both hydrogen atoms are bonded to one of the two nitrogen atoms.arrow_forwardDraw Lewis structures showing all valence electrons for these molecules. (a) C2H6 (b) CS2 (c) HCNarrow_forwardDraw Lewis structures to illustrate the covalent bonding in the following diatomic molecules. a. Cl2 b. HCl c. BrCl d. ClFarrow_forward
- Without actually drawing the Lewis structure, determine how many valence electrons are available for covalent bonding in each of the following molecules. a. CBr4 b. SF2 c. PH3 d. OF2arrow_forwardDraw Lewis structures to illustrate the covalent bonding in the following diatomic molecules. a. Br2 b. HBr c. BrF d. IBrarrow_forwardFor each row in the table below, decide whether the pair of elements will form a molecular compound held together by covalent chemical bonds. If the elements will form a molecular compound, check the box and enter the chemical formula and name of the compound. (If the elements will form more than one molecular compound, use the compound with the fewest total number of atoms.) You may assume all chemical bonds are single bonds, not double or triple bonds. element #1 element #2 hydrogen magnesium fluorine fluorine nitrogen bromine 44°F Explanation Cloudy element pair will form a molecular compound Check 0 0 molecular compound chemical formula 0 0 name 000 O Search 00 3 Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 99+ ⠀arrow_forward
- For each row in the table below, decide whether the pair of elements will form a molecular compound held together by covalent chemical bonds. If the elements will form a molecular compound, check the box and enter the chemical formula and name of the compound. (If the elements will form more than one molecular compound, use the compound with the fewest total number of atoms.) You may assume all chemical bonds are single bonds, not double or triple bonds. element #1 element #2 hydrogen nitrogen calcium fluorine iodine oxygen element pair will form a molecular compound molecular compound chemical formula 0 0 name 0 П 0 ×arrow_forwardFor each row in the table below, decide whether the pair of elements will form a molecular compound held together by covalent chemical bonds. If the elements will form a molecular compound, check the box and enter the chemical formula and name of the compound. (If the elements will form more than one molecular compound, use the compound with the fewest total number of atoms.) You may assume all chemical bonds are single bonds, not double or triple bonds. element #1 element #2 sodium carbon hydrogen fluorine bromine bromine element pair will form a molecular compound molecular compound chemical formula 0 0 name 0 П 0 Śarrow_forwardFor each row in the table below, decide whether the pair of elements will form a molecular compound held together by covalent chemical bonds. If the elements will form a molecular compound, check the box and enter the chemical formula and name of the compound. (If the elements will form more than one molecular compound, use the compound with the fewest total number of atoms.) You may assume all chemical bonds are single bonds, not double or triple bonds. element #1 element #2 calcium nitrogen hydrogen bromine nitrogen hydrogen element pair will form a molecular compound 0 molecular compound chemical formula name 1 □ 4 X 8 Śarrow_forward
- TT T In the first column type the number of atoms in the covalent compound. In the second column, type the total number of VALENCE electrons in the compound (all electrons: shared and unshared electrons). In the third column, determine the total number of possible chemical bonds in the compound. Compound H₂ Cl₂ 0₂ N₂ H₂O SF₂ CH4 NH3 PF3 CC14 CHEMISTRY Covalent Compounds and Electrons C₂H6 Number of Atoms Total Valence Electrons BHE Total possible of chemical bondsarrow_forwardwww TT In the first column type the number of atoms in the covalent compound. In the second column, type the total number of VALENCE electrons in the compound (all electrons: shared and unshared electrons). In the third column, determine the total number of possible chemical bonds in the compound. Compound H₂ Cl₂ 0₂ N₂ H₂O SF2 CH4 NH3 PF3 CC14 C₂H6 CHEMISTRY Covalent Compounds and Electrons Number of Atoms I Total Valence Electrons Total possible of chemical bondsarrow_forwardCovalent bonding involves the sharing of electrons between atoms. The number of covalent bonds an atom can form relates to the number of electrons it can share and still result in a neutral molecule. It is important to know how many bonds certain elements are most likely to form in order to draw structural formulas for molecules.arrow_forward
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