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Chemistry Unit 5

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Chapter 5

Chapter 5. Nomenclature. Systematic Naming. There are too many compounds to remember the names of them all. Compound is made of two or more elements. Put together atoms. Name should tell us how many and what type of atoms. Atoms and ions. Atoms are electrically neutral.

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e - Config. and Orb. Diag. for Ions

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compound, ions and formula

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Ionic Equilibria III: The Solubility Product Principle

20. Ionic Equilibria III: The Solubility Product Principle. Chapter Goals. Solubility Product Constants ?????? Determination of Solubility Product Constants ???????? Uses of Solubility Product Constants Fractional Precipitation ????

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by Steven S. Zumdahl & Donald J. DeCoste University of Illinois

Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois. Chapter 15 Solutions. Solutions. Solutions are homogeneous mixtures.

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Solutions Chapter 14

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Ionic Compounds and Naming

Ionic Compounds and Naming. Chapter 4.10,4.11 and 5. When we begin combining elements we make compounds. Two types Non-metal and metal Non-metal and non-metal Each type has unique physical and chemical properties Look at non-metal and metal in detail now and non-metal and non-metal later.

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Classifier Review

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Factoring Isotope Patterns A + 2 Elements (O, S and Si)

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Argentometric Titration (Precipitation Titration)

Argentometric Titration (Precipitation Titration). Meeting 7. Analite + Titrant ??? precipitation ? AgNO 3 ? ARGENTOMETRy. Principles: sedimentation of Ag(I) reaction. Diffuculties of titration: Hard to find the suitable indicators

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Solubility Equilibria

Solubility Equilibria. The Reality Behind the Solubility Rules. Solubility Rules- Qualitative solubility Equilibrium- Quantitative.

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Ionic Compounds: Writing Formulas

Ionic Compounds: Writing Formulas. Empirical Formulas. smallest whole-number ratio of elements in the compound Ionic compounds have empirical formulas only. Identify the empirical formulas. H 2 O H 2 O 2 CaF 2 NaCl CH 4 C 2 H 6 NiO FeCl 3. Empirical. Molecular. Empirical and Ionic.

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Chloride Analysis

Chloride Analysis. Chloride Methods. Gravimetric Chloride Potentiometric titration Visual Indicators Mohr Method Fajans Method Volhard Method. In all of these methods the chloride sample is dissolved & reacted with silver nitrate. Cl -1 + Ag +1 ? AgCl. Gravimetric Chloride.

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Jump Jump

Criss-cross notes. Jump Jump. Criss-Cross Method. Criss-cross is a _________ to help you find chemical __________ when you _________ atoms. shortcut. formulas. combine. **Formulas contain both the ________ in a compound and the _______ of that element. elements. amount. How Many?.

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Review for TEST on Chapter 2

Review for TEST on Chapter 2. Measurement. Density. Density = mass/volume; units g/mL or g/cm 3 . If mass is smaller, and volume is unchanged, predict what happens to density? If mass is unchanged, and volume is decreased, predict what happens to density?

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Warm-up 11/9/09

Warm-up 11/9/09. No, I did not get your exams graded ? Welcome to chemistry week! Does this equation violate the law of conservation of mass? NaCl + MgO ? Na 2 O + MgCl 2. Agenda 11/9/09. Formula worksheet Notes on balancing equations Learning Goal:

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Balancing Equations Chapter 6

Balancing Equations Chapter 6. What is balancing an equation?. Balancing an equation is changing the ratios of molecules/atoms to make the lowest possible same whole number and type of atoms on each side of the equation. Na + Cl 2 ? NaCl. 2. 2. What you can not do!.

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3.6 Molar Concentration

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Abstract

Seasonal variability in the growth rates of euphausiids from the northern Gulf of Alaska. A.I. Pinchuk * , R.R. Hopcroft, K.O. Coyle Institute of Marine Science, University of Alaska Fairbanks, AK 99775-7220 *e-mail: ftaip1@uaf.edu. Abstract

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