Reactions Reference. Solubility Rules 1.All nitrates, acetates, and chlorates are soluble. 2.All chlorides, bromides, and iodides are soluble except for.

Slides:

Advertisements

Similar presentations

How to predict a Product

Advertisements

 Single Replacement Reactions + + . General Equation A + BX  AX + B.

Reactions in Aqueous Solutions

Solubility Rules and Precipitation Reactions. Not all ionic compounds dissolve! Instead of doing experiments all the time to see which ones will dissolve,

Names and Formulas For Ionic Compounds

Phosphate. aluminum acetate Al 3+ hydrogen carbonate.

Precipitates and Solubility

Solubility Rules From the university of south Carolina

FORMULAS hydroxideOH -. FORMULAS sulfateSO 4 2- FORMULAS sulfiteSO 3 2-

Single & Double Replacement, Synthesis and Decomposition

Types of Chemical Reactions Synthesis (Combination) reaction Decomposition reaction A Single-replacement reaction B Double-replacement reaction Neutralization.

Oxidation: any process by which an entity loses electrons. e.g.2Mg o + O 2 o 2Mg 2+ + O 2- H 2 o + F 2 o 2H + F - Mg and H are oxidised in these examples.

Bell Work Write the electron configuration for an element with an atomic number of 23. Then, draw the electrons in their proper orbitals.

Identify the symbol: 1.Fluorine 2.Argon 3.Cesium 4.Barium 5.Antimony 6.Copper 7.Calcium 8.Potassium.

Review.  Cu +  Copper (I)  Tin (IV)  Sn 4+  Dichromate  Cr 2 O 7 2-

Ionic Compounds Nomenclature. Introduction We use the periodic table to tell us the most commonly expected charges for the ions of elements. For example:

Precipitation Reactions ● A reaction in which two solutions are mixed an insoluble solid (precipitate) is formed – Double replacement – ions switch partners.

Net Ionic Equations (8-4) Show only the species (atoms/ions) participating in a reaction o Single displacement reaction – exchange electrons o Double displacement.

Activity Series A method for predicting reactions.

 Determine the type of reaction and predict the products: NaOH  Li + Br 2  C 2 H 4 + O 2 

Solubility Rules. The terms soluble and insoluble are relative terms. soluble insoluble solute Solubility: the maximum amount of solute needed to make.

Polyatomic Ions. Common Polyatomic Ions Ion Name Ion Name NH 4 + ammonium nitrite nitrate phosphate hydrogen phosphate dihydrogen phosphate carbonate.

Net Ionic Equations And A Little Review.

13.2a Developing a Redox table.  the relative reactivity of metals can be used to determine which redox reactions are spontaneous In all redox reactions,

Chapter 8 Outline 8.1 – Chemical Equations The symbols and formulas used to represent reactants and products.

Ionic Bonding (Part IV)

Ions: Naming Practice SNC2D. F-F-F-F- F - Fluoride.

NaCl (aq) + Mg(NO3)2 (aq)  NaNO3 (aq) + MgCl2 (aq) 2

Ions: Naming Practice SNC2D. F-F-F-F- F - Fluoride.

CH 8 Solubility Rules & Net Ionic Equations. Chemical Reactions Many chemical reactions take place in solution. This means that the ionic compounds are.

Types of Chemical Reactions SynthesisSynthesis (Combination) reaction DecompositionDecomposition reaction Single-replacementSingle-replacement reaction.

Li K Ca Na Mg Al Zn Fe Pb H Cu Hg Ag Au Most Reactive Least Reactive F Cl B r I.

Ch 8 Single replacement reactions  A + BX  AX + B  You will have a chart of activity series  More active metals will replace less active metals from.

a. atoms are not created or destroyed in chemical reactions. (Atomic theory – Unit 3) b. The conservation of atoms: = # and type of atoms on the left.

The Activity Series & Solubility The Activity Series Ranks metals from most to least reactive. –the top are most reactive –the bottom are least reactive.

Ionic Bonding (Part 3) The Last Step: Adding Polyatomic Ions.

Balancing Equations Interactive Bonding learner.org.

Solubility Rules and Precipitation Reactions

ACT Prep Passage II 5 minutes Start when the bell rings

Chemistry 141 Monday, October 2, 2017 Lecture 12

Bell Ringer Complete and balance each of the following synthesis reactions by writing chemical equations. a. Na + O2→ ______ b. Mg + F2 → ______ a. 4Na.

Single Replacement, Double Replacement and Combustion Reactions

Christopher Whitehead Sixth Form:

Mixed Ion Flash Cards.

Single Replacement Reactions

Predicting Reactions.

Activity Series Foothill Chemistry.

Ionic Compounds.

DO NOW Pick up notes. Get out Balancing and Classifying Chemical Reactions from Monday. Word Equations: A Second Chance is due Friday – for a grade. Types.

Predicting Reactions.

Reaction Prediction What you MUST know before you even begin trying to predict a reaction: Element names & symbols Know your diatomics Oxidation states.

Types of Chemical Reactions

Clicker #1 When lead(II) nitrate and potassium iodide are mixed, what precipitate will form? Pb(NO3)2(aq) + KI(aq) → A) KNO3 B) KI C) Pb(NO3)2 D) PbI2.

Formation of a solid AgCl

Clicker #1 When lead(II) nitrate and potassium iodide are mixed, what precipitate will form? Pb(NO3)2(aq) + KI(aq) → A) KNO3 B) KI C) Pb(NO3)2 D) PbI2.

Speed Dating Speed Dating H Na Speed Dating Speed Dating K Be.

Types of Reactions There are FIVE main types of chemical reactions

Clicker #1 When lead(II) nitrate and potassium iodide are mixed, what precipitate will form? Pb(NO3)2(aq) + KI(aq) → A) KNO3 B) KI C) Pb(NO3)2 D) PbI2.

Common Polyatomic Ions

Friday Bellwork Predict the products of the following reactions and balance the equation. Ca + N2  Cl2 + Fe (iron III)  MgO + CO2.

Dissolve, Dissociate, Ionize, Precipitate

DETECTION LIMITS < 1 ppt ng/L 1-10 ppt ng/L ppt ng/L

Section 3: Transition Metal Ions

Predicting Products: single & double replacement reactions

HMSA Get Polarity pgs stamped Today: get through page 22

Ionic Compound Formulas

Predicting the Product in Single Replacement Reactions

Increase in Ease of Oxidation

Group 1 Group 2 Group 3 Group 5 Group 4 Ag+, Pb2+, Hg22+

Clicker #1 When lead(II) nitrate and potassium iodide are mixed, what precipitate will form? Pb(NO3)2(aq) + KI(aq) → A) KNO3 B) KI C) Pb(NO3)2 D) PbI2.

Presentation transcript:

Reactions Reference

Solubility Rules 1.All nitrates, acetates, and chlorates are soluble. 2.All chlorides, bromides, and iodides are soluble except for Ag +, Hg 2 2+, and Pb 2+ 3.All sulfates are soluble except for Ca 2+, Sr 2+, Hg 2 2+, Pb 2+, and Ag + 4.All carbonates, chromates, sulfites, and phosphates are insoluble except those of group I and NH All hydroxides are insoluble except for those of group I and lower II 6.All sulfides except those of the I and II groups are insoluble 7.Salts containing a group I metal or the ammonium ion are soluble

Activity series of the Metals Li Rb K Ba Sr Ca Na Mg Al Mn Zn Cr Fe Cd Co Ni Sn Pb H2 Sb Bi Cu Hg Ag Pt Au

Activity Series of the Nonmetals F 2 Cl 2 Br 2 I 2