Homework Help is Here – Start Your Trial Now!
Science
Chemistry
gold (I) bicarbonate manganese (IV) hypochlorite lithium sulfide aluminum iodate bismuth (III) nitrate sulfurous acid chromium (III) chloride rubidium periodate copper (II) sulfate tin (II) carbonate heptachlorine difluoride

gold (I) bicarbonate manganese (IV) hypochlorite lithium sulfide aluminum iodate bismuth (III) nitrate sulfurous acid chromium (III) chloride rubidium periodate copper (II) sulfate tin (II) carbonate heptachlorine difluoride

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question

Nomenclature

Purpose: To practice naming and writing formulas of ionic compounds and to learn about molecular compounds and their naming. Introduction: Part 1: Ionic compounds By now you have watched this week's videos on naming compounds and writing formulas. This is simply more practice! There are a few ions in the report sheet that you probably haven't seen before. However, we can draw some parallels to help us remember. We know Cl Chloride Clo Нуроchlorite Clo, Chlorite ClO, Chlorate Clo, Perchlorate We can follow this pattern above for other halogens like bromine and iodine. Br Bromide Iodide BrO Нуpobromite IO Нуpoiodite BrO, Bromite IO2 Iodite BrO; Bromate IO3 Iodate BrO4 Perbromate IO4 Periodate There are more similarities observed within families on the periodic table. Both sulfur and selenium form similar bonds with oxygen: SO," is sulfate; SeO, is selenate. Phosphorus and arsenic also form analogous ions with oxygen, such as phosphate, PO,", and arsenate, ASO,*. Part 2: Molecular Compounds Molecular compounds (also sometimes called covalent compounds) are made up of all nonmetals. We will focus on the binary molecular compounds in this lab, meaning ones that are made of only two elements. Since nonmetals are on the right side of the periodic table, in order to reach octet they have to gain electrons. When creating a compound from these elements, we are putting together atoms that all want to have extra electrons and nobody wants to give up any electrons. How can this be accomplished? By sharing! The important consequence of sharing electrons is that they are no longer traded between atoms; if electrons are not added or removed, there are no charges that could help us figure out how to put the atoms together in a formula correctly. Instead, we have to rely on names. When naming molecular compounds we have to use prefixes to indicate how many atom there are. The prefixes are Mono- 1 Неха- Di- Нepta- 7 Tri- 3 Octa- 8 Tetra- 4 Nona- 9. Penta- 5 Deca- 10 The rest of naming is straight forward. We name the first element by its name, then the second element ending in -ide. Finally, we go back and add prefixes that correspond to the number of atoms in that compound. Examples: N2O4 There are 2 nitrogen atoms and 4 oxygen atoms in this molecule. So the name is dinitrogen tetroxide. Note that "a" from tetra is sometimes dropped to simplify pronunciation. P,O10 There are 4 phosphorus atoms and 10 oxygen atoms in this molecule. The name is tetraphosphorus decaoxide. Cl207 There 2 chlorine atoms and 7 oxygen atoms in this molecule. The name is dichlorine heptaoxide. Procedure: Now it's time to practice! Name and write formulas for ionic and molecular compounds in the report sheet. The ones that say “skip" are acids and they follow a different naming convention all together, so don't worry about those. I can't emphasize enough how important it is to be able to write formulas and names correctly and how much easier and smoother the rest of the semester will go if we get really good at this from the start.
Transcribed Image Text:Purpose: To practice naming and writing formulas of ionic compounds and to learn about molecular compounds and their naming. Introduction: Part 1: Ionic compounds By now you have watched this week's videos on naming compounds and writing formulas. This is simply more practice! There are a few ions in the report sheet that you probably haven't seen before. However, we can draw some parallels to help us remember. We know Cl Chloride Clo Нуроchlorite Clo, Chlorite ClO, Chlorate Clo, Perchlorate We can follow this pattern above for other halogens like bromine and iodine. Br Bromide Iodide BrO Нуpobromite IO Нуpoiodite BrO, Bromite IO2 Iodite BrO; Bromate IO3 Iodate BrO4 Perbromate IO4 Periodate There are more similarities observed within families on the periodic table. Both sulfur and selenium form similar bonds with oxygen: SO," is sulfate; SeO, is selenate. Phosphorus and arsenic also form analogous ions with oxygen, such as phosphate, PO,", and arsenate, ASO,*. Part 2: Molecular Compounds Molecular compounds (also sometimes called covalent compounds) are made up of all nonmetals. We will focus on the binary molecular compounds in this lab, meaning ones that are made of only two elements. Since nonmetals are on the right side of the periodic table, in order to reach octet they have to gain electrons. When creating a compound from these elements, we are putting together atoms that all want to have extra electrons and nobody wants to give up any electrons. How can this be accomplished? By sharing! The important consequence of sharing electrons is that they are no longer traded between atoms; if electrons are not added or removed, there are no charges that could help us figure out how to put the atoms together in a formula correctly. Instead, we have to rely on names. When naming molecular compounds we have to use prefixes to indicate how many atom there are. The prefixes are Mono- 1 Неха- Di- Нepta- 7 Tri- 3 Octa- 8 Tetra- 4 Nona- 9. Penta- 5 Deca- 10 The rest of naming is straight forward. We name the first element by its name, then the second element ending in -ide. Finally, we go back and add prefixes that correspond to the number of atoms in that compound. Examples: N2O4 There are 2 nitrogen atoms and 4 oxygen atoms in this molecule. So the name is dinitrogen tetroxide. Note that "a" from tetra is sometimes dropped to simplify pronunciation. P,O10 There are 4 phosphorus atoms and 10 oxygen atoms in this molecule. The name is tetraphosphorus decaoxide. Cl207 There 2 chlorine atoms and 7 oxygen atoms in this molecule. The name is dichlorine heptaoxide. Procedure: Now it's time to practice! Name and write formulas for ionic and molecular compounds in the report sheet. The ones that say “skip" are acids and they follow a different naming convention all together, so don't worry about those. I can't emphasize enough how important it is to be able to write formulas and names correctly and how much easier and smoother the rest of the semester will go if we get really good at this from the start.
Lab 5 - Nomenclature gold (I) bicarbonate diboron nonachloride manganese (IV) hypochlorite nickel (II) phosphate lithium sulfide rubidium bromate aluminum iodate rubidium hydrogen sulfite bismuth (III) nitrate titanium (III) oxalate sulfurous acid Skip iodine octanitride chromium (III) chloride Iron (III) hydroxide rubidium periodate manganese (II) cyanide copper (II) sulfate titanium (III) sulfite tin (II) carbonate diselenium decabromide heptachlorine difluoride lead (IV) chlorite bismuth (V) nitrite Iron (II) hypoiodite iodic acid Skip beryllium hypobromite hydrogen cyanide mercury (I) cyanide potassium nitride lead (II) sulfide octacarbon heptachloride chromium (III) iodate mercury (II) phosphide magnesium bicarbonate bismuth (III) hypoiodite cobalt (II) phosphide gold (III) hydroxide decaboron decafluoride pentaphosphorus pentaiodide Lead (II) chromate cobalt (II) carbide permanganic acid skip hydrogen fluoride cobalt (II) selenide calcium phosphate pentasulfur octaiodide silver cyanide chromium (II) carbide hydrocyanic acid skip calcium bromate bismuth (III) sulfide hexaselenium monoxide
Transcribed Image Text:Lab 5 - Nomenclature gold (I) bicarbonate diboron nonachloride manganese (IV) hypochlorite nickel (II) phosphate lithium sulfide rubidium bromate aluminum iodate rubidium hydrogen sulfite bismuth (III) nitrate titanium (III) oxalate sulfurous acid Skip iodine octanitride chromium (III) chloride Iron (III) hydroxide rubidium periodate manganese (II) cyanide copper (II) sulfate titanium (III) sulfite tin (II) carbonate diselenium decabromide heptachlorine difluoride lead (IV) chlorite bismuth (V) nitrite Iron (II) hypoiodite iodic acid Skip beryllium hypobromite hydrogen cyanide mercury (I) cyanide potassium nitride lead (II) sulfide octacarbon heptachloride chromium (III) iodate mercury (II) phosphide magnesium bicarbonate bismuth (III) hypoiodite cobalt (II) phosphide gold (III) hydroxide decaboron decafluoride pentaphosphorus pentaiodide Lead (II) chromate cobalt (II) carbide permanganic acid skip hydrogen fluoride cobalt (II) selenide calcium phosphate pentasulfur octaiodide silver cyanide chromium (II) carbide hydrocyanic acid skip calcium bromate bismuth (III) sulfide hexaselenium monoxide
Expert Solution
Introduction

When two or more atoms combine with each other, they will form molecule and those molecules has different formula called molecular formula. Every molecule has different molecular formula with different physical and chemical properties.

trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Green Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS