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This document discusses ionic compounds and how they are formed and named. When atoms gain or lose electrons to form ions, they are called cations if positively charged or anions if negatively charged. Ionic compounds are named by writing the metal first followed by the nonmetal, such as calcium chloride (CaCl2) where calcium is the metal cation and chloride is the nonmetal anion. Polyatomic ions, groups of atoms that behave as a single unit with a charge, are also included in ionic compound names such as iron (III) sulfate (Fe2(SO4)3) where sulfate is the polyatomic anion.
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- Properties of salts like high melting points and conductivity are discussed briefly.
- The basics of Lewis dot structures and molecular geometry are introduced for covalent bonding in organic compounds. Electronegativity and molecular polarity are also covered.
_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.
Net ionic equations
The document discusses net ionic equations, which involve writing molecular and ionic equations and identifying spectator ions. A molecular equation shows all species as whole units, while an ionic equation shows dissolved species as free ions. To write a net ionic equation, the molecular equation is first written and balanced, then molecules are broken into ions. Spectator ions that are present on both sides of the reaction are then canceled to give the net ionic equation. The document also discusses what substances will ionize or dissociate into ions in solution based on their type (salt, acid, base) and whether they are considered strong electrolytes.
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.
Ionic Naming
The document provides information on naming ionic compounds, cations, anions, and polyatomic ions. It discusses how to name monatomic and transition metal cations by adding "-ion" or the charge in Roman numerals after the element name. Anions are named by adding "-ide" after the element root. Ionic compounds are formed by writing the cation first followed by the anion. Polyatomic ions are also included.
GENCHEM1-nomenclature.pptx
Nomenclature is the process of naming chemical compounds with systematic names so they can be easily identified. This document discusses the naming of ionic compounds, including binary ionic compounds composed of a metal and nonmetal, and ternary ionic compounds containing a polyatomic ion. It explains that the cation is always named first and the anion name ends in "-ide" for binary ionic compounds. For transition metals, Roman numerals indicate the ion charge. Ternary compounds contain two ions, with at least one being a polyatomic ion, and both ions are simply named in order.
IB Chemistry on Redox, Oxidizing, Reducing Agents and writing half redox equa...
This document provides a tutorial on redox reactions, oxidation states, and half reactions. It begins by defining redox as involving both oxidation and reduction, which is the loss or gain of electrons. It then discusses oxidation states (also called oxidation numbers), which are assigned to atoms in compounds to keep track of electrons. Rules are provided for assigning oxidation states based on electronegativity. Redox reactions involve a change in oxidation states between reactants and products. Examples of assigning oxidation states to elements in compounds are also given.
Building molecules
a detailed set of solutions to textbook problems related to simple molecule compounds. diagrams, problems, text.
Electrochemical series
The document discusses three tables that are part of an electrochemical series. Table 1 lists standard reduction potentials alphabetically by element symbol. Table 2 lists reactions with positive potentials relative to the hydrogen electrode, in order of increasing potential. Table 3 lists reactions with negative potentials relative to the hydrogen electrode, in order of decreasing potential. The document notes that the reliability of the potentials varies and some values may be revised occasionally.
Electrochemical series
The document discusses three tables that provide standard reduction potentials (E° values) for various electrochemical reactions. Table 1 lists elements alphabetically by symbol. Table 2 lists reactions with positive E° values relative to the standard hydrogen electrode, in order of increasing potential. Table 3 lists reactions with negative E° values relative to the standard hydrogen electrode, in order of decreasing potential. The document notes some reactions have more reliable E° values than others based on number of significant figures.
IB Chemistry on Redox, Oxidizing, Reducing Agents and writing half redox equa...
The document discusses oxidation numbers (also called oxidation states), which are used to keep track of electrons in chemical reactions. Some key points:
- Oxidation numbers are assigned to each atom in a chemical species by assuming ionic bonding and counting electrons.
- Common rules are outlined for assigning oxidation numbers to elements, such as metals in Group 1 have a +1 oxidation state and nonmetals in Group 7 have a -1 oxidation state.
- Oxidation numbers can be used to determine if a reaction is a redox reaction by looking for changes in oxidation numbers between reactants and products.
- Transition metals can have multiple common oxidation states. Roman numerals are used to distinguish, such as
PP_15a_chp_2_8_naming_ionic_compounds.ppt
The document discusses naming simple ionic compounds. It provides rules for naming type I and type II binary ionic compounds. For type I compounds, the cation is named first followed by the anion with the "-ide" suffix. For type II compounds containing metals with multiple charges, the roman numeral for the metal's charge is included in parentheses. The document also discusses naming compounds containing polyatomic ions by following similar rules.
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- 1. IONIC COMPOUNDS By Ken Costello
- 2. + _ battery compass Coil of wire + _ What’s an ion? Let’s find out…
- 3. + _ battery compass Coil of wire Copper Chloride + _ Switch is open. Nothing happening yet.
- 4. + _ battery compass Coil of wire Copper Chloride If copper atoms are going to the negative side, what charge do they have? What about the chlorine atoms? + _
- 5. + _ battery compass Coil of wire Copper Chloride + + + + Since the atoms wandered towards each side, let’s call them IONS from the Greek word, ion, meaning wanderer . + _
- 6. + _ Copper Chloride CuCl 2 + + + Also, since the positive side of a battery is called the anode (way up) , we’ll call ions that go towards it anions . + + + + + Since the negative side of a battery is called the cathode (way down) , we’ll call ions that go towards it cations . anode anode cathode cathode + _ Anions Cations
- 7. IA IIA IIIA VIA VA IVA +4 +1 +2 +3 -4 -2 -1 -3 0 VIIA VIIIA Naming compounds by taking a metal from groups 1A, 1B, or 1C , and combining with a non-metal .
- 8. Understanding how ions react to other elements will help in naming compounds or coming up with formulas for the compounds.
- 10. IA IIA IIIA VIA VA IVA +1 +2 +3 2e - 3p + 4p + Li Be B 5p + 6p + C VIIA VIIIA How do you know the charge? +4 -4
- 11. IA IIA IIIA VIA VIIA VA IVA +4 VIIIA +1 +2 +3 -2 -1 -3 -4 0 2e - N O F 7p + 8p + 9p + 10p + Ne 8e - Na 11p +
- 12. IA IIA IIIA VIA VA IVA +4 +1 +2 +3 -4 2e - 4p + Be -2 -1 -3 0 +2 2e - F 9p + -1 VIIA VIIIA
- 13. IA IIA IIIA VIA VA IVA +4 +1 +2 +3 -4 -2 -1 -3 0 VIIA VIIIA 2e - 4p + Be +2 2e - F 9p + -1 2e - F 9p + -1
- 14. IA IIA IIIA VIA VA IVA +4 +1 +2 +3 -4 -2 -1 -3 0 BeF 2 VIIA VIIIA Berylium Fluoride Be +2 F -1 F -1
- 15. For ionic compounds with a metal from group 1A, 2A, & 3A place the metal first and name it first. The non-metal is put last and named last. The number of metals or non-metals is depends on how many it takes to balance the charges. +1 +2 -2 -1 -3 IA IIA IIIA VIA VA IVA VIIA VIIIA
- 16. IA IIA IIIA VIA VA IVA +4 +1 +2 +3 -4 -2 -1 -3 0 Al +3 Cl -1 AlCl 3 VIIA VIIIA Aluminum Chloride Cl -1 Cl -1 Al +3 Cl -1
- 17. IA IIA IIIA VIA VA IVA +4 +1 +2 +3 -4 -2 -1 -3 0 Fe +3 O -2 Fe 2 O 3 VIIA VIIIA O -2 O -2 Fe +3 O -2 Fe +3 Fe Fe O O O
- 19. IA IIA IIIA VIA VA IVA +4 +1 +2 +3 -4 -2 -1 -3 0 Zn +2 NO 3 -1 Zn(NO 3 ) 2 VIIA VIIIA Zinc = +2 NO 3 -1 NO 3 -1 Zn +2 O N O O Zn O N O O
- 20. IA IIA IIIA VIA VA IVA +4 +1 +2 +3 -4 -2 -1 -3 0 Fe +3 SO 4 -2 Fe 2 (SO 4 ) 3 VIIA VIIIA Iron=+3 Now called Iron(III) sulfate SO 4 -2 SO 4 -2 Fe +3 Fe +3 SO 4 -2 O O S O O O O S O O Fe O O S O O Fe