Imagine we combine the substances shown to the right: 8. Which of the following products is likely to form? a) b) OH CH₂ONa -O Na* c) d) HINT: Na+ is a cation (CH3O¯ is an anion) a C

The atomic number of sulfur is 16. Sulfur combines withhydrogen by covalent bonding to form a compound, hydrogensulfide. Based on the number of valence electrons in a sulfuratom, predict the molecular formula of the compound.(A) HS(B) HS2(C) H2S(D) H4S

Question 2 28. Write Lewis structures for the following: and answer the following questions about the Lewis structure (a) H2 how many bonds? [ Select ] (c) PCI3 how many lone pairs on P? [ Select] (d) SF2 how many lone pairs on S? Select] (e) H2CCH2 how many bonds between the carbon atoms? [Select ] a 99+ ho 近

Predict which of these compounds are ionic and which are covalent.(A) Ca3N2(B) Li2CO3(C) PCl5(D) NaOH(E) CH4(F) MgO

From their positions in the periodic table, arrange the atoms in each of the following series in order of increasing electronegativity:(a) As, H, N, P, Sb(b) Cl, H, P, S, Si(c) Br, Cl, Ge, H, Sr(d) Ca, H, K, N, Si(e) Cl, Cs, Ge, H, Sr

2. Draw the Lewis structures for each of the following ions or molecules. Give the number of electrons in each species. Remember to enclose ions in square brackets with the charge as a superscript outside the right bracket. (a) Br 20 (c) BrF 3 (e) PCI 4* (b) IOF 3 (I is the central atom) (d) ASF 3

3. Using electronegativity difference, indicate the type of bond between the following atoms: (a) Li-Cl(b) C-Br(c) F-Cl(d) Br-Br

#6. Consider the Lewis structure below where X is an element from the third period (Na-Ar). (a) Identify the central atom, X, when n = - -1. (b) Determine the formal charge on X. (c) Draw a Lewis structure so that the formal charge on X is equal to +1. :Ö: [+] n-

Name each ionic compound. In each of these compounds, the metal forms only one type of ion. (a) Lil (b) MgS (c) BaF2 (d) NaF

Ionic Bonding 1. Show the transfer of electrons with ↓ notation in the reactions between the following pairs of elements to create an ionic compound. Show the elements as atoms, even though they may exist as diatomic or polyatomic species. (a) Ba and F (b) K and I (c) Cs and S (d) Ca and As (e) Li and N (f) Rb and Se (g) Sr and P (h) Al and Br 2. Write Lewis dot structures for atoms and ions of each of the reactants and products in Exercise 1.