Concept explainers
(a)
Interpretation:
The Lewis symbols for the lithium atom has to be determined.
Concept Introduction:
Lewis electron-dot symbols can be used to predict the number of bonds formed by most elements in their compounds. Lewis electron-dot symbol consists of the chemical symbol for an element surrounded by dots that represent its valence electrons.
Some features of the Lewis electron-dot symbol are as follows:
1. It is the representation of valence electrons.
2. It allows to keep track of valence electrons during bond formation.
3. It consists of the chemical symbol for the element and a dot for each valence electron.
(b)
Interpretation:
The Lewis symbol for
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The Lewis symbol for
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
The Lewis symbol for bromine atom has to be determined.
Concept Introduction:
Refer to part (a).
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Chemistry: Principles and Practice
- Which of the following compounds has both ionic and covalent bond? (a) H2O (b) NH4Cl (c) NaCl (d) HClarrow_forward2. 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 3arrow_forwardii. Answer true or false. (a) A covalent bond is formed between two atoms whose difference in electronegativity is less than 1.9. (b) If the difference in electronegativity between two atoms is zero (they have identical electronegativities), then the two atoms will not form a covalent bond. (c) A covalent bond formed by sharing two electrons is called a double bond. (d) In the hydrogen molecule (H2), the shared pair of electrons completes the valence shell of each hydrogen. (e) In the molecule CH4, each hydrogen has an electron configuration like that of helium, and carbon has an electron configuration like that of neon. (f) In a polar covalent bond, the more electronegative atom has a partial negative charge (8-) and the less electronegative atom has a partial positive charge (&+). (g) These bonds are arranged in order of increasing polarity C-Harrow_forwardWrite the Lewis structures for the following, and include resonance structures where appropriate. Indicate which has the strongest carbon-oxygen bond.(a) CO2(b) COarrow_forwardNa+ forms an “ionic bond” (i.e. an electrostatic attraction) with the OCN− ion. (a) Draw the full Lewis structure of the ionic compound. Be sure to show how you have derived this. (The ionic compound as a whole, not just OCN-) (b) Which atom in the OCN− anion is the sodium cation most likely to attract? Explain.arrow_forwardAn elemental analysis of a hydrocarbon, which contains only carbon and hydrogen, shows the mass%: element mass% carbon 92.26 hydrogen 7.743 (A) * Determine the empirical formula of the hydrocarbon. (B) The compound has a molar mass of 26.04 g/mol. Determine its molecular formula. (C, Draw the Lewis structure of the molecular compound. Count the total number of sigma bonds and pi bonds each, present in the molecule. (D, What is the hybridization of carbon in the molecule? Explain.arrow_forwardWrite Lewis dot symbols for the following atoms and ions: (a) I (b) I-(c) S(d) S2-(e) P (f) P3-(g) Na (h) Na+(i) Mg (j) Mg2+arrow_forwardNa+ forms an “ionic bond” (i.e. an electrostatic attraction) with the OCN− ion. (a) Draw the full Lewis structure of the ionic compound. Be sure to show how you have derived this. (b) Which atom in the OCN− anion is the sodium cation most likely to attract? Explain.arrow_forwardWrite an electron configuration for each element and the corresponding Lewis structure. Indicate which electrons in the electron configuration are included in the Lewis structure.(a) N(b) C(c) Cl(d) Ararrow_forwardAnswer true or false. (a) The octet rule refers to the chemical bonding patterns of the first eight elements of the Periodic Table. (b) The octet rule refers to the tendency of certain elements to react in such a way that they achieve an outer shell of eight valence electrons. (c) In gaining electrons, an atom becomes a positively charged ion called a cation. (d) When an atom forms an ion, only the number of valence electrons changes; the number of protons and neutrons in the nucleus does not change. (e) In forming ions, Group 2A elements typically lose two electrons to become cations with a charge of 12. (f) In forming an ion, a sodium atom (1s22s22p63s1) completes its valence shell by adding one electron to fill its 3s shell (1s22s22p63s2). (g) The elements of Group 6A typically react by ac- cepting two electrons to become anions with a charge of 22. (h) With the exception of hydrogen, the octet rule applies to all elements in periods 1, 2, and 3. (i) Atoms and the ions derived from…arrow_forwardPredict which of these compounds are ionic and which are covalent.(A) Ca3N2(B) Li2CO3(C) PCl5(D) NaOH(E) CH4(F) MgOarrow_forwardConsider the following compounds: BeCl 2 , MgBr 2 , and SrBr 2 . Answer the following questions based on expected periodic trends: (a) Which is expected to have the shortest ionic bonds? (b) Which is expected to have the highest lattice energy? (c) Which is expected to have the lowest melting point?arrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_forward_ios
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning