Short quiz 2 Chemistry
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The document contains a short quiz asking students to: 1. Write the chemical formulas for potassium nitrate, sodium sulphate, and copper(II) sulphate. 2. Write the chemical equation for the reaction between magnesium carbonate and hydrochloric acid, which forms magnesium chloride, water, and carbon dioxide. 3. Identify the anion in phosphide ion and the cation in magnesium ion from multiple choice options.
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Short quiz 1 Chemistry
The document contains a short chemistry quiz asking the student to:
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3) Write the chemical equation for the reaction of sodium with oxygen producing a metallic oxide.
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This document discusses different types of inorganic compounds including oxides, hydrides, bases/hydroxides, acids, and salts. Oxides are binary compounds formed when metals combine with oxygen or nonmetals combine with oxygen. The document then provides an activity that asks the reader to select various compounds and classify them as either metal or nonmetal oxides.
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This document discusses the chemical analysis of salts. It explains that some salts decompose when heated, showing a change in color and releasing gases. The ease with which a salt breaks down determines its thermal stability. Carbonate and nitrate salts decompose in different ways when heated, such as forming metal oxides, carbon dioxide, oxygen, or ammonia, depending on the reactivity of the metal. Most sulphate and chloride salts do not decompose with heat except for ammonium chloride. Physical properties like solubility and color can be used to identify salts. Anions and cations in aqueous solutions can be identified using characteristic tests that involve adding reagents like sodium hydroxide or ammonia.
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The document contains a short chemistry quiz asking the student to:
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2) Write the chemical formulas for calcium chloride, aluminum oxide, and sodium hydroxide.
3) Write the chemical equation for the reaction of sodium with oxygen producing a metallic oxide.
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SUBJECT - CHEMISTRY
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This document discusses different types of inorganic compounds including oxides, hydrides, bases/hydroxides, acids, and salts. Oxides are binary compounds formed when metals combine with oxygen or nonmetals combine with oxygen. The document then provides an activity that asks the reader to select various compounds and classify them as either metal or nonmetal oxides.
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This document discusses the chemical analysis of salts. It explains that some salts decompose when heated, showing a change in color and releasing gases. The ease with which a salt breaks down determines its thermal stability. Carbonate and nitrate salts decompose in different ways when heated, such as forming metal oxides, carbon dioxide, oxygen, or ammonia, depending on the reactivity of the metal. Most sulphate and chloride salts do not decompose with heat except for ammonium chloride. Physical properties like solubility and color can be used to identify salts. Anions and cations in aqueous solutions can be identified using characteristic tests that involve adding reagents like sodium hydroxide or ammonia.
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The document provides examples of precipitation reactions showing the formation of precipitates. It discusses how lead hydroxide, iron(III) hydroxide, iron(II) hydroxide, copper hydroxide, and lead(II) iodide precipitates are formed through various reactions. It also addresses which ions cannot be identified using precipitation reactions and which ions can form hydroxides that dissolve in excess sodium hydroxide.
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The document provides examples of precipitation reactions showing the formation of precipitates. It discusses how lead hydroxide, iron(III) hydroxide, iron(II) hydroxide, copper hydroxide, and lead(II) iodide precipitates are formed through various reactions. It also addresses which ions cannot be identified using precipitation reactions and which ions can form hydroxides that dissolve in excess sodium hydroxide.
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2) Instructions for students on completing the paper.
3) Sample questions covering topics in chemistry like thermodynamics, equilibrium, redox reactions, organic chemistry and biomolecules.
4) A value based question assessing students' ability to apply chemistry knowledge to an ethical scenario.
Nomenclature
This document provides information on naming and writing formulas for various types of compounds including:
- Ionic compounds formed from cations and anions
- Molecular compounds formed from nonmetals
- Acids
It discusses common names versus IUPAC names, determining charges on ions, writing formulas to balance charges, and using prefixes to indicate the number of atoms in molecular compounds. Examples are provided to illustrate each type of nomenclature.
7BC Nomenclature
This document provides examples of chemistry questions and answers related to naming and drawing structures of ionic and covalent compounds. It includes the electron dot structures and formulas for magnesium chloride (MgCl2) and sulfur dioxide (SO2). Additionally, it provides examples of subquestions that could be asked to assess understanding of ionic bonding concepts such as determining ion charges based on group numbers.
_orcututgk_Naming Compounds-Chemistry.ppt
1. The document discusses naming ionic and covalent compounds. It provides steps for naming ionic compounds, which involve writing the name of the metal ion and nonmetal ion. Covalent compounds are named by writing the names of the nonmetals and adding prefixes to indicate ratios.
2. Binary covalent compounds are between two nonmetals and are named using prefixes like mono, di, and tri to show ratios of elements. Polyatomic ions are also named and used in ionic compounds.
3. Determining if a compound is ionic or covalent depends on whether it contains a metal and nonmetal (ionic) or only nonmetals (covalent).
Naming Compounds-Chemistry.ppt
This document provides instructions for naming ionic and binary covalent compounds. It explains that ionic compounds are formed from metals and nonmetals, while covalent compounds contain only nonmetals. The naming process for ionic compounds involves writing the name of the metal ion followed by the nonmetal ion changed to -ide. For covalent compounds, prefixes are used to indicate the number of each nonmetal present. Practice problems are provided to name compounds and write formulas.
Naming and Writing Formula of Compounds.pptx
This document provides instructions for naming ionic and binary covalent compounds. It explains that ionic compounds are formed from metals and nonmetals, while covalent compounds contain only nonmetals. The naming process for ionic compounds involves writing the name of the metal ion followed by the nonmetal ion changed to -ide. For covalent compounds, prefixes are used to indicate the number of each nonmetal present.
Tema 4 the chemical compounds
This document provides information about chemical compounds and their nomenclature. It defines a chemical compound as a pure substance formed by two or more elements combined in fixed proportions. Examples of common compounds and their chemical formulas are provided. The document then discusses different systems for naming compounds, including classical nomenclature, nomenclature using Roman numerals to indicate elemental valence, and nomenclature using Greek prefixes to indicate the number of atoms present. Specific rules and examples are provided for naming oxides, hydroxides, and peroxides. A series of exercises are included to have the reader practice writing formulas and names according to the various nomenclature systems.
Naming compounds chemistry
The document provides instructions for naming ionic and binary covalent compounds. Ionic compounds are formed from metals and nonmetals, with the metal ions taking positive charges and the nonmetal ions taking negative charges. Binary covalent compounds are formed from two nonmetals sharing electrons in ratios indicated by prefixes like di-, tri-, and tetra-. The naming process for ionic compounds involves writing the name of the metal ion followed by the name of the nonmetal ion. For binary covalent compounds, the process involves writing the names of the two nonmetals, changing the second to end in "-ide", and adding prefixes to indicate ratios.
10 naming and formula writing 2012
This document provides information on naming and writing formulas for various types of chemical compounds including:
1) Binary ionic compounds consisting of a metal and non-metal are named by writing the metal followed by the non-metal with "ide" ending. The chemical formula is written with the symbols.
2) Ionic compounds with multivalent metals or polyatomic ions are named using prefixes like "ous" and "ic". Formulas include charges in parentheses.
3) Molecular compounds of non-metals are named by writing the non-metals with the second element having an "ide" ending. Prefixes are converted to subscripts in formulas.
Nomenclature
The document provides information on naming and writing formulas for various types of chemical compounds including:
1. Ionic compounds formed from cations and anions are named by writing the metal first followed by the nonmetal with the appropriate ending (e.g. NaCl is sodium chloride).
2. Molecular compounds formed from nonmetals use prefixes to indicate the number of atoms and the second element takes the "-ide" ending (e.g. CO2 is carbon dioxide).
3. Acids are named by identifying if they contain one or two elements and whether they contain oxygen, and using appropriate endings like "-ic", "-ous", or specifying the anion (e.g. HCl is hydrochlor
F.Sc.2.Chemistry.Ch.2.Test Solved-Malik Xufyan ...
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- 1. NAME : CLASS : SHORT QUIZ 2 1. Write the formula ion 2. Write down the chemical formula of the following substance: i. Potassium nitrate - _______________ ii. Sodium sulphate - _______________ iii. Copper (II) sulphate - _______________ 3. Write down the chemical equation of the following reactions i. Chemical reaction between magnesium carbonate, MgCO3, and dilute hydrochloric acid, HCl. Magnesium Chloride, MgCl2, water and carbon dioxide are formed. No Formula ion Anion 1 Phosphide ion 2 Hydroxide ion 3 Dichromate(VI) ion 4 Manganate(VII) ion 5 Phosphate ion No Formula ion Cation 1 Magnesium ion 2 Calcium ion 3 Aluminum ion 4 Copper (II) ion 5 Zinc ion
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