Arrange the compounds below in decreasing order of the ionic character of the bonds in them. That is, pick 1 for the compound with the most ionic bonds, pick 2 for the compound with the next most ionic bonds, and so on. ionic character of bonds compound CIF (Choose one) Periodic Table F2 (Choose one) ▼ NaF (Choose one) ▼ SF2 (Choose one)

Arrange the compounds below in decreasing order of the ionic character of the bonds in them. That is, pick 1 for the compound with the most ionic bonds, pick 2 for the compound with the next most ionic bonds, and so on. ionic character of bonds compound CIF (Choose one) Periodic Table F2 (Choose one) ▼ NaF (Choose one) ▼ SF2 (Choose one)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Covalent and ionic compounds can be differentiated easily because of their 2. Usually ionic compound b. metalic compound d. both a and b What I Can Do Covalent and ionic compounds can be differentiated easily because of th different physical properties based on the nature of their bonding. Fill-in the blank whether it is covalent or ionic compound based on the properties: When (1) Ionil Compound are formed, we are almost never dealing with just a single positive ion andla single negative ion. The process of gaining and losing electrons completely changes the chemical properties of a substance. The chemical and physical properties of an (2) Joni ompound will bear no resemblance to the properties of the elements which formed the ions. Some elements, however, can achieve an octet in a different way by sharing their valence (3). (4). electrons, are unable to achieve an octet by electron sharing. electrons with other atoms and this Typically, only non-metals are able to form Metals, with…
For each row in the table below, decide whether the pair of elements will form a molecular or ionic compound. If they will, then enter the chemical formula of the compound. If the elements will form more than one compound, enter 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 compound formed? chemical formula ionic iodine cesium O molecular ? neither jonic hydrogen охудen O molecular O neither O ionic calcium sodium O molecular neither
Answer the questions in the table below about the shape of the sulfur dioxide (SO₂) molecule. How many electron groups are around the central sulfur atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central sulfur atom? (You may need to use the scrollbar to see all the choices.) 0 (choose one) O
In each of the molecules drawn below one chemical bond is colored red. Decide whether this bond is likely to be polar or not. If the bond is likely to be polar, write down the chemical symbol for the atom which will have more negative charge. : 0: H - H Br: 0=C=0 - : 0: C1: The highlighted bond is polar and the more negative atom is The highlighted bond is nonpolar. The highlighted bond is polar and the more negative atom is The highlighted bond is nonpolar. The highlighted bond is polar and the more negative atom is The highlighted bond is nonpolar.
The valence electrons configuration of X is ns? and Y is ns²np³. What is the most likely chemical formula of the compound made from these elements? O X3Y2 O XY3 O XY2 O XY
(ii) Complete the following Lewis structure and answer the questions below it. H H H H -C- 0-CEN What is the empirical formula of this compound? How many lone pairs of electrons that this compound have? How many multiple bonds does this compound have? How many nonbonding electrons does this compound have? How many molecules are in 15.0 mg of this compound? How many bonding pairs of electrons does this compound have? How many polar bonds does this compound have? What is the VSEPR formula for the nitrogen atom at the end of the molecule?
Complete the table to indicate the number of covalent bonds, lone pairs, and valence electrons around each atom in the O molecule shown. : 0: H Atom Covalent bonds Lone pairs Valence electrons C о Cl H Which atoms in the molecule fulfill the octet rule? H Cl
Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure Is the proposed Lewis structure reasonable? ○ Yes. : 0: H- =0 =0 : C : 0: No, it has the wrong number of valence electrons. The correct number is: ☐ No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* O Yes. O No, it has the wrong number of valence electrons. The correct number is: ☐ No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* O Yes. O No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* * If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many times as necessary. For example, if two oxygen atoms don't satisfy the octet rule, enter "O,O". X G
Arrange the single covalent bonds within each set in order of INCREASING polarity. If: • most polar is b • medium polarity is c • least polar is a this leads to the following input: acb (To answer this question you may consult the table of electronegativity values in the table below.) 1A 2A Li Be 1.0 1.5 Na Mg 0.9 1.2 3B 4B 5B 6B 7B K 0.8 1.0 1.3 Ca Sc Ti V Cr Mn Fe 1.5 1.6 1.6 1.5 1.8 Rb 0.8 Sr 1.0 Y 1.2 <1.0 1.0-1.4 1. a) C-H b) P-H c) Br-H Cs Ba La Hf Ta W Re Os 0.7 0.9 1.1 1.3 1.5 1.7 1.9 2.2 2. a) P-H b) O-H c) N-H Zr 1.4 1.6 1.8 1.9 2.2 H 2.1 1.5-1.9 2.0-2.4 8B Nb Mo Te Ru Rh 8222=2 Co Ni 1.8 1.8 2.5-2.9 3.0-4.0 Pd 2.2 Pt 2.2 3A 4A 5A 6A 7A B C N 0 F 2.5 2.0 3.0 3.5 4.0 Al 1.5 1B Cu 1.9 1.6 1.6 2B Zn Ga Ge 1.8 Au Hg 2.4 Si P S CI 1.8 2.1 2.5 3.0 Ag Cd In Sn 1.9 1.7 1.7 1.8 TI Pb 1.9 1.8 1.8 As Se Br 2.0 2.4 2.8 Sb Te I 1.9 2.1 2.5 Bi Po At 1.9 2.0 2.2
Arrange the compounds below in decreasing order of the ionic character of the bonds in them. That is, pick 1 for the compound with the most ionic bonds, pick 2 for the compound with the next most ionic bonds, and so on. compound MgO Na₂O 0₂ NO₂ ionic character of bonds (Choose one) (Choose one) (Choose one) (Choose one) X Ś
Using the answers to the questions attached answer the question: Why are compounds composed of integer ratios of elements?
Group 1 elements have an average electronegativity of 0.84 (not including hydrogen). Group 17 elements have an average electronegativity of 2.99. These two groups often form bonds. Given this information, which kind of bond will they form? * Periodic Table of the Elements He Li Be C Ne Na Mg Al SI CI Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd in Sn Sb Xe Hf Ta Re Os Ir Pt Au Hg TL Pb Po At Rn Cs Ba Fr Ra Db Sg Bh Hs Mt Ds Rg Cn Nh FL Mc Lv Ts Og Rf Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Cf Es Fm Md No Lr Ac Th Pa Np Pu Am Cm Bk