Concept explainers
(a)
Interpretation:
A soft, waxy solid that consists of carbon and hydrogen only has to be classified as ionic or non-ionic based on the name or description.
Concept Introduction:
Ionic compounds:
An atom or a molecule having a net electrical charge is known as ion. Charge of the electron is negative and charge of the proton is positive. Both electron and proton have the same magnitude. Positively charged ion is called cation and negatively charged ion is called anion. Because of the opposite charge of cation and anion they will readily form ionic compounds. Ions consisting of only a single atom known as monoatomic ions and more than two atoms form polyatomic ions.
(b)
Interpretation:
The substance ammonium oxalate has to be classified as ionic or non-ionic.
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
A hard, brittle solid that melts above
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
An alkali metal oxide has to be classified as ionic or non-ionic.
Concept Introduction:
Refer to part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 2 Solutions
Chemistry: The Molecular Science
- Use your knowledge of the correct number of covalent bonds to predict the formula for a simple compound formed between bromine and the following elements. (Enter NONE if no compound is likely to form.) (a) phosphorus (b) carbon (c) nitrogen (d) hydrogenarrow_forwardName each ionic compound. In each of these compounds,the metal forms only one type of ion. (a) CsCl (b) SrBr2 (c) K2O (d) LiFarrow_forward1) Using principles of chemical bonding and/or intermolecular forces, explain each of the following. (a) Xenon has a higher boiling point than neon has. (b) Solid copper is an excellent conductor of electricity, but solid copper chloride is not. (c) SiO2 melts at a very high temperature, while CO2 is a gas at room temperature, even though Si and C are in the same chemical family. (d) Molecules of NF3 are polar, but those of BF3 are not. 2) Using principles of chemical bonding and/or intermolecular forces, explain each of the following: (a) MgCl2 and SiCl4 (b) MgCl2 and MgF2 (c) F2 and Br2 (d) F2 and N2 Note: Please Briefly Explainarrow_forward
- Assume that you encounter the following phrases in your reading. What is the chemical formula for each substance mentioned? (a) Sodium Hydrogen carbonate is used as a deodorant. (b) Calcium hypochlorite is used in some bleaching solutions. (c) Hydrogen cyanide is a very poisonous gas. (d) Magnesium hydroxide is used as a cathartic. (e) Tin (II) fluoride has been used as a fluoride additive in toothpastes. (f) When cadmium sulfide is treated with sulfuric acid, fumes of hydrogen sulfide are given off.arrow_forwardWhich of the following compounds has both ionic and covalent bond? (a) H2O (b) NH4Cl (c) NaCl (d) HClarrow_forwardWrite a feature which will distinguish a metallic solid from an ionic solid.arrow_forward
- (A) CsBr (B) MgCl2arrow_forwardWrite formulas for the compounds:(i) iodic acidarrow_forward1.Draw the electronic diagrams for the following compounds (showing outermost shell electrons only). (a) A compound formed from calcium and sulphur (b) a compound formed from aluminium and oxygen (c) A compound formed from nitrogen and chlorine (d) carbon dioxidearrow_forward
- Name each ionic compound. In each of these compounds, the metal forms more than one type of ion. (a) CrCl2 (b) C:CI3 (c) SnO2 (d) Pbl2arrow_forwardPredict which of these compounds are ionic and which are covalent.(A) Ca3N2(B) Li2CO3(C) PCl5(D) NaOH(E) CH4(F) MgOarrow_forwardIodine monochloride and elemental bromine have nearly the same molar mass and liquid density but very different boiling points. (a) What molecular property is primarily responsible forthis difference in boiling point? What atomic property gives rise to it? Explain. (b) Which substance has a higher boiling point?Why?arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning