2.E: Atoms, Molecules, and Ions- Homework
- Page ID
- 360576
For Chapter 2 you MUST know:
- The names and symbols for elements 1-36
- Know the polyatomic Ions. You MUST know ammonium (\(\ce{NH4+}\)), acetate ( \(\ce{CH_3COO^-}\)), carbonate ( \(\ce{CO_3^{2-}}\)), hydroxide ( \(\ce{OH^-}\)), nitrate ( \(\ce{NO_3^-}\)), phosphate ( \(\ce{PO_4^{3-}}\)), and sulfate ( \(\ce{SO_4^{2-}}\)).
Turn in your answers for the following questions - show your work
- How many protons, neutrons and electrons are present in one atom of the following:
- 1H
- 2H
- 3H
- 79Br
- 81Br1-
- 262Bh
- What is the Atomic Weight of chlorine given that:
- The exact mass of 35Cl is 34.9689 and the relative abundance is 75.53%
- The exact mass of 37Cl is 36.9659 and the relative abundance is 24.47%
- Is this the answer that you expected?
- What is the Atomic Weight of ruthenium given the following information from WebElements, www.webelements.com. Is this the answer that you expected?
- Isotope Abundance Exact Mass
- 96Ru 5.54% 95.907599
- 98Ru 1.87% 97.905287
- 99Ru 12.76% 98.9059389
- 100Ru 12.60% 99.9042192
- 101Ru 17.06% 100.9055819
- 102Ru 31.55% 101.9043485
- 104Ru 18.62% 103.905424
- For the following molecules; write the chemical formula.
- carbon dioxide
- iron (II) chloride
- dinitrogen pentoxide
- iron (III) sulfate
- Name the following compounds.
- KI
- CaF2
- Cu2SO4
- N2O
- LiOH
- Give the chemical formula (or atomic symbol) and charge for the following ions:
- sulfate
- sulfite
- nitrate
- chloride
- nitride
- acetate
- carbonate
The Following Questions are for your practice - Do Not Turn In. They include answers so you can check your work
2.3: Atomic Structure and Symbolism
- Write the symbol for each of the following ions:
- the ion with a 1+ charge, atomic number 55, and mass number 133
- the ion with atomic number 15, mass number 31, and a 3− charge
(a) 133Cs+; (b) 31P3−
- Give the number of protons, electrons, and neutrons in neutral atoms of each of the following isotopes:
- \(\ce{^7_3Li}\)
- \(\ce{^{125}_{52}Te}\)
(a) 3 protons, 3 electrons, 4 neutrons; (b) 52 protons, 52 electrons, 73 neutrons
2.4: Chemical Formulas
Write the molecular and empirical formulas of the following compounds:
(a)
(b)
(a) molecular CO2, empirical CO2; (b) molecular C2H2, empirical CH
2.5: The Periodic Table
Using the periodic table, classify each of the following elements as a metal or a nonmetal, and then further classify each as a main-group (representative) element, transition metal, or inner transition metal:
- uranium
- bromine
- gold
- americium
(a) metal, inner transition metal; (b) nonmetal, representative element; (c) metal, transition metal; (d) metal, inner transition metal
2.6: Molecular and Ionic Compounds
Using the periodic table, predict whether the following chlorides are ionic or covalent: KCl, NCl3, ICl, and PCl5.
Ionic: KCl; Covalent: NCl3, ICl, PCl5
2.7: Chemical Nomenclature
Name the following compounds:
- CsCl
- BaO
- K2S
(a) cesium chloride; (b) barium oxide; (c) potassium sulfide;
Write the formulas of the following compounds:
- rubidium bromide
- magnesium selenide
- calcium chloride
(a) RbBr; (b) MgSe; (c) CaCl2
Write the formulas of the following compounds:
- chlorine dioxide
- dinitrogen tetraoxide
- potassium phosphide
- silver(I) sulfide
(a) ClO2; (b) N2O4; (c) K3P; (d) Ag2S
Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds:
- Cr2O3
- FeCl2
- CrO3
(a) chromium(III) oxide; (b) iron(II) chloride; (c) chromium(VI) oxide