Nomenclature 1.

Slides:



Advertisements
Similar presentations
Making Chemical Compounds
Advertisements

LECTURE 5 CHM 151 ©slg TOPICS: 1. Naming Cations 2. Naming Anions 3. Naming Ionic compounds 4. Naming Molecular Binary Compounds.
Polyatomic Ions & Chemical Nomenclature Meyer 2013.
Chapter 7: Chemical Nomenclature
Chemical Names and Formulas
“When I see a cation, I see a positive ion;
Chapter 5 Types of Compounds
Ch. 8: Nomenclature Naming of compounds. ● Metals and non-metals combine to form ionic compounds ● Non-metals and non-metals combine to form molecular.
IonicCovalentMetallic Chemical Bonds  e- transfer  Crystal lattice  ions  Na + Cl Na + Cl -  “salts”  very strong bonds generally between metals.
Acetate CH 3 COO -. Chlorate ClO 3 - Chlorite ClO 2 -
Salts Containing Polyatomic Ions Acids Oxyacids HW: Read 4-4 &4-6 Do problems 32, 34, 47, & 48 on pgs
Chemical Compounds Honors Chemistry.
Polyatomic Nomenclature.  In polyatomic compounds, a positive ion and negative ion attract one another to form an ionic bond.  To write formulas for.
A. Element vs. Compound Element Cannot be chemically broken down into two different substances. - Atoms of all the same type Compound Combination of elements.
Naming Chemicals. Binary Ionic compounds Definitions Binary Ionic Compound- compound containing two elements—one metal and one non-metal + Cation + Cation.
Naming and Formula Writing What’s in a name?. Quick Review What do metals want to do? –So what do they become? What do nonmetals want to do? –So what.
Assigning Oxidation States The concept of oxidation numbers (or oxidation states) was devised as a simple way of keeping track of electrons in reactions.
Ionic Compound Molecular Compound Ionic Compounds are the result of oppositely charged ions attracting to each other after an electron transfer has occurred.
Covalent Bonds and Molecular Geometry
Nomenclature and writing chemical equations
Naming Compounds Writing Formulas and Equations
The language of chemistry
Ionic Bonding and Ionic Compounds
CHEMICAL NAMES & FORMULAE
Chemical Nomenclature
Molecular Compounds & Acids
More on Chemical Compounds Nomenclature
Super Duper Cheat Sheet for Naming Compounds
6/18/2018 Naming Compounds Part 2.
Element and Ion Review Given the name, supply the formula and charge (if applicable). Given the formula, supply the name. You will have 10 seconds to respond.
Naming Acids & Bases.
Names & Formulas Nomenclature.
Chemical Names and Formulas
Naming Compounds: cations and anions
Chapter 4 Nomenclature.
Chemical Nomenclature
Chapter 9 Chemical Names and Formulas Section 9.1 Naming Ions
Unit 4 Chemical Formulas Ionic Molecular Cation (+) Anion (-) No ions
10/23/09 Naming Compounds Day 2.
Day 71 Notes (Ch. 17 & 20) Electrolytes, Acids and Bases.
Naming Compounds and Writing Formulas
Chemical Names and Formulas
BEWARE!!! There is a lot memorization involved with this chapter.
Cpt 7 Chemical formulas.
Chapter 3 Molecules, Compounds, and Chemical Equations
POLYATOMIC IONS tightly bound groups of atoms that behave as a unit and carry a charge most end in –ite or –ate exceptions: NH4+ – ammonium CN– – cyanide.
Naming Compounds and Writing Formulas
Chapter 7 Chemical Formulas & Chemical Compounds
Chapter 5 Nomenclature.
Naming Inorganic Compounds
TOPIC 0D: Nomenclature.
Chemical Names & Formulas
More Nomenclature.
Naming the Inorganic Compounds
Warm-Up What is an ion? How is it formed?.
Chapter 9 Chemical Names and Formulas
Chapter 2 Atoms, Molecules, and Ions
Chemical Names and Formulas
Ch. 6 Notes---Chemical Names & Formulas
Chemical Bonding and Nomenclature
Nomenclature Chapter 9.
Lesson 3.2 – Naming Compounds
Naming Compounds Writing Formulas
Naming Compounds Writing Formulas and Equations
Chemical Nomenclature
Chapter 2 The Material World
Nomenclature Naming Compounds.
5/23/2019 Naming Compounds Day 2.
Chapter 6 Language of Chemistry by Christopher G. Hamaker
Writing Formulas Chemistry 7(B)
Presentation transcript:

Nomenclature 1

Bonds Ionic Covalent Metallic Chemical Bonds “glue”

Ionic Bonds + - e- transfer Crystal lattice ions Na + Cl Na+ Cl - “salts” very strong bonds generally between metals and non metals. Solids at room temp. Very high melting points Ex: NaCl Tmp = 1074K Poor conductors of electricity in a solid state + -

Covalent Bonds . orbital overlap sharing “molecules” hypothetical charge H + H H H . orbital overlap Bonding e- are localized between two atoms Formed between two nonmetals

Metallic Structure “sea” of e- e- are delocalized

Nomenclature of Binary Compounds

Ionic Compounds

Ionic Examples

Ionic Compounds with Transition Metals

Transition Metal Examples

Molecules: Covalent Bonded Compounds

Binary Molecule Examples

Assigning Oxidation States The concept of oxidation numbers (or oxidation states) was devised as a simple way of keeping track of electrons in reactions. We use the following rules for assigning oxidation numbers: Free Elements (Na, O2, etc.) 0 Group 1 Elements in a compound1 +1 Group 2 Elements in a compound +2 Group 3 Elements in a compound +3 “O” in a compound2 -2 “F” in a compound -1 1Exception to this rule occurs for hydrogen in hydrides (e.g. LiH, where the oxidation state of hydrogen is –1). 2Exception to this rule occurs in peroxides (e.g. H2O2, where the oxidation state of oxygen is –1).

NOTE: Three transition metals, Cd2+, Zn2+ and Ag+, are understood to exist in these oxidation states (numbers); therefore, Roman numerals are NOT included in parentheses. Also note that the mercury(I) ion is written as a diatomic ion (dimer): Hg2+2. WorkShop Determine the oxidation state of each underlined atom: KMnO4, ClO4-, and S2O32-.

Common Polyatomic Ions – YOU MUST MEMORIZE THESE!!! Acetate C2H3O2- Hydroxide OH-Ammonium NH4+ Hydrogen sulfate HSO4- Carbonate CO32- Hydrogen phosphate HPO42- Chromate CrO42- Nitrate NO3- Hypochlorite ClO- Nitrite NO2- Chlorite ClO2- Oxalate C2O42- Chlorate ClO3- Permanganate MnO4- Perchlorate ClO4- Peroxide O22- Cyanide CN- Phosphate PO43- Dichromate Cr2O72- Sulfate SO42- Dihydrogen phosphate H2PO4- Sulfite SO32- Hydrogen carbonate HCO3- Thiocyanate SCN-

Polyatomic Ion Examples

Naming Acids Two main types of acids (this class) Binary Acids – certain compounds of Hydrogen with other nonmetal atoms. Examples: HClO hypochlorous acid HClO2 chlorous acid HClO3 chloric acid HClO4 perchloric acid HNO2 nitrous acid HNO3 nitric acid 2. Oxoacids – Hydrogen with two other nonmetals, one of which is oxygen. Examples: HF (aq) Hydrofluoric acid HCl (aq) Hydrochloric acid HBr (aq) Hydrobromic acid HI (aq) Hydroiodic acid H2S (aq) Hydrosulfuric acid

Acid Naming Examples

Naming Hydrates and Simple Organic Compounds Hydrates are ordinary chemical substances that have associated with them a certain number of water molecules. For example, CuSO45H2O is read copper(II) sulfate pentahydrate. As we will see in section 2, when determining the overall molecular weight of this particular compound, you ADD five water molecules to the initial CuSO4 (as opposed to multiply, where the “” is commonly misinterpreted by beginner chemistry students; more on this later)! When dealing with organic (or carbon-containing) compounds, we refer to the following prefixes: Number of Carbons Prefix 1 Meth- 2 Eth- 3 Prop- 4 But- 5 Pent- 6 Hex- 7 Hept- 8 Oct- 9 Non- 10 Dec-

Naming Simple Organic Compounds Compounds containing only carbon and hydrogen are called hydrocarbons. Hydrocarbons that contain only carbon-carbon single bonds are called alkanes. The simplest alkane is methane (CH4), followed by ethane (C2H6 or CH3CH3), etc. The names of the alkanes are composed of two parts: a prefix indicating the number of carbon atoms, and the suffix “-ane” indicating that the molecule contains only carbon-carbon single bonds. Hydrocarbons that contain only carbon=carbon double bonds are called alkenes. The simplest alkene is ethene (C2H4 or CH2CH2) followed by propene (C3H6).

Simple Organic Molecules

Workshop on Nomenclature 1. Name each of the following compounds: A. KClO4 G. KMnO4 B. Ca3(PO4)2 H. K2Cr2O7 C. Al2(SO4)3 I. CH3CH2CH2CH2CH3 D. Pb(NO3)2 J. Li2C2O4 E. BaSO3 K. TiO2 F. NaNO2 L. BaCl28H2O 2. Name each of the following compounds: A. NaCl G. NO B. MgCl2 H. NaHSO4 C. RbBr I. N2F4 D. CsF J. FePO4 E. AlI3 K. SiF4 F. V2O5 L. Ca(HSO3)2

Workshop continued: 3. Write formulas for the following compounds: A. potassium dichromate G. ammonium acetate B. sulfur hexafluoride H. ammonium hydrogen sulfate C. sodium dihydrogen phosphate I. cobalt(III) nitrate D. lithium nitride J. mercury(I) chloride E. chromium(III) carbonate K. potassium chlorate F. octane L. cobalt(II) chloride heptahydrate 4. Write formulas for the following compounds: A. sodium hydroxide G. potassium hypochlorite B. aluminum hydroxide H. lead(IV) oxide C. hydrogen cyanide I. ammonium chromate D. sodium peroxide J. copper(I) bromide E. copper(II) acetate K. germanium dioxide F. carbon tetrafluoride L. butane

5. The formulas and common names for several substances are given below. What are the systematic names for these substances? A. sugar of lead Pb(C2H3O2)2 B. blue vitrol CuSO4 C. quicklime CaO D. milk of magnesia Mg(OH)2 E. laughing gas N2O 6. Writing Names and Formulas of Compounds i. Write the formula of each of the following compounds. A. Calcium hydroxide ____________________ B. Nickel(II) phosphate ____________________ C. Beryllium iodide ____________________ D. Chromium(III) sulfide ____________________ E. Diphosphorus tetroxide ____________________ F. Aluminum oxide ____________________ G. Ammonium nitrate ____________________ H. Phosphorus pentachloride _________________

ii. Name each of the following compounds. A. Na3PO4 ________________________________ B. PF5 ________________________________ D. FeBr3 ________________________________ E. Cu2O ________________________________ F. Cr(OH)3 ________________________________ G. Rb2SO4 ________________________________ H. N2O ________________________________ I. HI ________________________________ J. KH ________________________________ K. Cr2O3 ________________________________ L. MgSO46H2O ________________________________ M. CH3CH2CH3 ________________________________