A NaCl B Li C H2O D He E S Answer: A Diff: 1 Page Ref: 9. Answer: There should be 3 equivalent resonance structures drawn, each containing 1 single Br-O bond and 2 double Br-O bonds. A N B O C Br D He Answer: C Diff: 2 Page Ref: 9. The dash - represents two dots. If the result are small structures they will be molecular eg 1 and 4 in your list.
Determine the total number of valence electrons in a molecule 2. Compoiunds of this type usually contain a metal elements joined to non-metal element - so compounds 2 and 3 in your list are ionic. Answer: The Al should have no electrons around it, with a 3+ charge. Label each atom with its formal charge. The number of bonding sites is detemined by considering the number of valence electrons and the ability of an atom to expand it's octet. Structure B is more accurate because it has more formal charge on the atoms c.
Based on these electronegativities PbH4 would be expected to A be ionic and contain H- ions. E None of the above are exothermic. And that represents the best structure for ClO3-. A Li Cl B Na Cl C K Cl D Rb Cl Answer: A Diff: 2 Page Ref: 9. A 0 pairs B 1 pair C 2 pairs D 3 pairs E 4 pairs Answer: D Diff: 1 Page Ref: 9. Answer: F Diff: 1 Page Ref: 9. For instance, complete structures are more useful for the novice organic chemist learning to appreciate the mechanism of a reaction while simplified versions may be preferred by inorganic chemists.
E All of these compounds are equally stable according to Lewis theory. Answer: Dipole moment is the measured quantitative value associated with the separation of the partial positive and negative charges found within a molecule. A CaN B Ca3N2 C CaN2 D Ca2N E Ca2N3 Answer: B 8 Use Lewis theory to determine the chemical formula for the compound formed between Rb and S. Diff: 1 Page Ref: 9. Structure A is more accurate because the forma charge is 0 on each atom. So let's see what that does to our formal charges now that we've moved those in there to form a double bond.
The electron geometry will be the same because there are no unbonded pairs. Electronegativity is the strength of the attraction of a nucleus to a pair of shared bonding electrons within a covalent bond. D Single bonds are shorter than double bonds. E None of the above are true. A 1s22s22p63s24p6 B 1s22s22p63s23p6 C 1s22s22p63s23p5 D 1s22s23p64s25p6 E 1s22s2p63s2p6 Answer: B Diff: 3 Page Ref: 9. C Ionic compounds at room temperature typically conduct electricity. Answer: A pure covalent bond occurs when bonding electrons are shared equally or very close to it as in the N-N bond.
Lone pairs are in green. Search our 100 + Lewis Structures. A polar covalent bond is formed between 2 atoms of differing electronegativities. So we have 2, 4, 6, 8, 10, 12, 14, 16, and then back to the center, 18, and 20. Structure B is more accurate because it has more formal charge on the atoms c.
Answer: A 37 Which of the following elements can form compounds with an expanded octet? For instance in our example, N cannot expand its octet so keeps a formal charge of 1+ and both singly bonded oxygens a formal charge of 1-. Description Chemistry: A Molecular Approach, 2e Tro Chapter 9 Chemical Bonding I: Lewis Theory Multiple Choice Questions 1 Identify an ionic bond. A P-F B C-Br C C-F D C-I E C-Cl Answer: D 30 Using periodic trends, place the following bonds in order of increasing ionic character. A C-N B C-F C C-O D C-C E F-F Answer: B Diff: 1 Page Ref: 9. Beryllium goes in the centre. A NaCl B Li C H2O D He E S Answer: C Diff: 1 Page Ref: 9.
When the compound is made from only non-metal elements, electrons are not lost or gained but shared as these elements tend not to lose electrons or gain them. A single covalent bond B double covalent bond C triple covalent bond D all of the above bonds are the same length Answer: C Diff: 1 Page Ref: 9. A Rb2O B Sr O C In2O3 D C O2 Answer: C Diff: 2 Page Ref: 9. Depends on the need of the chemist. Lewis diagrams are drawn to examine mechanisms so knowing which parts of a molecule are electron defficient + and which are electron rich - is vital. Bond pairs are in purple. A B C D E Answer: B Diff: 1 Page Ref: 9.
A B C D E Answer: B 3 Which of the following represent the Lewis structure for Mg? Remember, Chlorine is in Period 3 and can hold more than 8 valence electrons. Answer: B Diff: 2 Page Ref: 9. Because P normally has 5 valence electrons and it is paired with 5 F atoms, it has no unbonded pairs. A AlN B MgO C NaF D CaS E RbI Answer: A Docsity. A S B Cl C Ti D Se Answer: B Diff: 1 Page Ref: 9.
Answer: Formal charge is the charge of an atom that it would have if all bonding electrons were shared equally between the bonded atoms. B partial negative δ- charge. A B C D E Answer: A Diff: 1 Page Ref: 9. Answer: A Diff: 1 Page Ref: 9. A H-I B H-Br C H-F D H-Cl E C-H Answer: C 29 Choose the bond below that is least polar. Transcript: Let's do the ClO3- Lewis structure.