Before you get started..................................
.......it is probably worth revising the fundamentals about The Atom and The Periodic Table.
.......it is probably worth revising the fundamentals about The Atom and The Periodic Table.
You might find The Periodic Table of Videos interesting to explore. You are NOT required the memorise the periodic table!! You will always have a copy in your tests and exam. However, if you feel you need some assistance becoming more familiar with the placement of some key elements the illustrated copies might be useful.
Getting started.......
To get started study pages 1-15 in the Essentials Workbook, answer the questions as you progress. Chapters 1, 2 & 3 in Discovering Chemistry have relevant further reading. Most of this should be revision. These materials will help you with the Periodic Table Assignment: Part A.
To get started study pages 1-15 in the Essentials Workbook, answer the questions as you progress. Chapters 1, 2 & 3 in Discovering Chemistry have relevant further reading. Most of this should be revision. These materials will help you with the Periodic Table Assignment: Part A.
Oxides can be tricky to get your head around. HINT: look for the patterns. There are only two types of general equations to know for each of acidic and basic oxides - if you pick up the pattern the rest is easy! We will discuss this more in class.
Below are the Key Ideas from the SACE Stage 2 Chemistry Subject Outline, this is what you should know after completing your study of this part of the course.
Key Ideas
The arrangement of electrons in any atom can be described in terms of shells and subshells.
The position of an element in the periodic table reflects its electron configuration.
The periodic table is the unifying framework for the study of the chemical elements and their compounds. Elements within each group of the periodic table have similar chemical properties that can be explained in terms of their similar outer-shell electron configurations.
The electronegativities of non-metallic atoms are higher than those of metals; non-metallic atoms tend to gain electrons in chemical reactions.
The trend from metallic to non-metallic behaviour across a period is related to the increase in electronegativity. These trends are reflected in changes in the acidic/basic character of the oxides.
The oxides of non-metals are acidic. Their acidic character can be displayed by reaction with hydroxide ions to produce an oxyanion and, in most cases, by reaction with water to produce an oxyacid.
The oxides of metals are basic. Their basic character can be displayed by reaction with an acid to produce a cation and, in some cases, by reaction with water to produce OH- in solution.
Metalloids form amphoteric oxides. Amphoteric oxides can display basic character by reaction with hydrogen ions and acidic character by reaction with hydroxide ions.
Key Ideas
The arrangement of electrons in any atom can be described in terms of shells and subshells.
The position of an element in the periodic table reflects its electron configuration.
The periodic table is the unifying framework for the study of the chemical elements and their compounds. Elements within each group of the periodic table have similar chemical properties that can be explained in terms of their similar outer-shell electron configurations.
The electronegativities of non-metallic atoms are higher than those of metals; non-metallic atoms tend to gain electrons in chemical reactions.
The trend from metallic to non-metallic behaviour across a period is related to the increase in electronegativity. These trends are reflected in changes in the acidic/basic character of the oxides.
The oxides of non-metals are acidic. Their acidic character can be displayed by reaction with hydroxide ions to produce an oxyanion and, in most cases, by reaction with water to produce an oxyacid.
The oxides of metals are basic. Their basic character can be displayed by reaction with an acid to produce a cation and, in some cases, by reaction with water to produce OH- in solution.
Metalloids form amphoteric oxides. Amphoteric oxides can display basic character by reaction with hydrogen ions and acidic character by reaction with hydroxide ions.
TOPIC CHECKLIST
After studying these concepts you should be able to...........................
Write, using subshell notation, the electron configuration of an atom or monatomic ion of any of the first thirty-eight elements in the periodic table.
Identify the s, p, d, and f block elements in the periodic table.
Predict the following properties of the s and p block elements of any of the first thirty-eight elements in the periodic table:
• metal, metalloid, or non-metal nature of the element
• charge of the monatomic ions
• likely oxidation number(s) of the element in its compounds (including octet expansion for phosphorus, sulfur, and chlorine).
Find regions in the periodic table with elements of high, intermediate, and low electronegativity.
Predict the acidic/basic character of the oxides of an element from the position of the element in the periodic table.
Write equations for the reactions of oxides of non-metals such as SiO2, CO2, SO2, SO3, and P4O10 with hydroxide ions and with water, where a reaction occurs.
Write equations for the reactions of oxides of metals such as MgO, Na2O, CuO, and Fe2O3 with acids and with water, where a reaction occurs.
Write equations for the reactions of amphoteric oxides such as Al2O3 and ZnO with hydrogen ions or hydroxide ions.
After studying these concepts you should be able to...........................
Write, using subshell notation, the electron configuration of an atom or monatomic ion of any of the first thirty-eight elements in the periodic table.
Identify the s, p, d, and f block elements in the periodic table.
Predict the following properties of the s and p block elements of any of the first thirty-eight elements in the periodic table:
• metal, metalloid, or non-metal nature of the element
• charge of the monatomic ions
• likely oxidation number(s) of the element in its compounds (including octet expansion for phosphorus, sulfur, and chlorine).
Find regions in the periodic table with elements of high, intermediate, and low electronegativity.
Predict the acidic/basic character of the oxides of an element from the position of the element in the periodic table.
Write equations for the reactions of oxides of non-metals such as SiO2, CO2, SO2, SO3, and P4O10 with hydroxide ions and with water, where a reaction occurs.
Write equations for the reactions of oxides of metals such as MgO, Na2O, CuO, and Fe2O3 with acids and with water, where a reaction occurs.
Write equations for the reactions of amphoteric oxides such as Al2O3 and ZnO with hydrogen ions or hydroxide ions.
Periodic Table Assignment: Part A - due Friday week 2
Just for fun..................
