'Simplest formula' diaporamas de présentation

TOPIC 5-CHEMICAL COMPOUNDS

TOPIC 5-CHEMICAL COMPOUNDS. CONTENTS Types of Chemical Compounds and Their Formulas The Mole Concept and Chemical Compounds Composition of Chemical Compounds Oxidation States Naming Chemical Compounds. CHEMICAL COMPOUNDS. They are composed of two or more different elements

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Chapter 1

Chapter 1. Be familiar with the metric system and its prefixes (conversion). Apply the rules for significant figures (and do not forget to use them after chapter 1). Chapter 1. Do not resist using conversion factors. They will be used over and over again throughout the course.

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Formulas, Equations, and Moles

Formulas, Equations, and Moles. Chapter 3. Molar Mass. The sum of the atomic masses for all the atoms represented in the chemical formula of a compound. AKA formula mass, molecular mass, molecular weight. Mole (mol). Number of particles in atomic mass in grams of an element.

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Chapter 10 Arrays and Functions

Chapter 10 Arrays and Functions. Prepared by: Lec . Ghader Kurdi. Arrays. Arrays are data structures which hold multiple variables of the same data type. Consecutive group of memory locations having same name and type ( int , char, float, double etc.).

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The Peasantry Before October

The Peasantry Before October . Classes and Categories within the Peasantry. Landowners Kulaks-own property (tools, cattle, some land) Highered landless peasants Muzhik (peasant) Farm hands-wage workers Renters- (like sharecroppers). Timeline of Tactics of Peasantry.

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Percentage Composition

If you have a box containing 100 golf balls and 100 ping pong balls, which type of ball contributes the most to the mass of the box? The same principle applies to finding the % composition of a compound. Different elements have different masses and this must be taken into consideration.

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EMPIRICAL FORMULA

EMPIRICAL FORMULA. Is the simplest whole-number ratio of atoms of each element present in a compound For example, the empirical formula of C 3 H 6 is CH 2 . If the mass of each element in a sample is known, then the empirical formula can be calculated. Steps to consider.

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Empirical & Molecular Formulas

Empirical & Molecular Formulas. Chapter 3. Mathematical Methods. STEP 1 Obtain in the laboratory, the number of grams OR the weight percentage of each element in the compound. This can be found by: breaking down the existing compound into its elements

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Warm-up

Warm-up. What is the empirical formula for C 6 H 6 ?. CH. What is the percentage composition of Hydrogen in C 6 H 12 O 6 ?. What is the percentage composition of Hydrogen in C 6 H 12 O 6 ? C: 12(6) = 72. What is the percentage composition of Hydrogen in C 6 H 12 O 6 ?

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Simplest formula calculations

Simplest formula calculations. Q- a compound is found to contain the following % by mass: 69.58% Ba , 6.090% C, 24.32% O. What is the simplest (i.e. empirical) formula?

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Simplest formula calculations

Simplest formula calculations. Q- a compound is found to contain the following % by mass: 69.58% Ba, 6.090% C, 24.32% O. What is the simplest (i.e. empirical) formula?

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CH 3 Mass Relations in Chemistry; Stoichiometry

CH 3 Mass Relations in Chemistry; Stoichiometry. Atomic Mass. Indicates how heavy an element is compared to another element. Units AMU---Atomic Mass Unit Defined as 1/12 of the mass of a C-12 atom. Atomic Mass from isotope composition. Isotopic Abundance: the natural of an isotope.

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The Mole

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Empirical Formulas

Empirical Formulas. Empirical formula tells the relative number of atoms of each element in a compound Mole concept provides a way of calculating the empirical formula Also called the simplest formula. Steps. Assume a 100g sample . Change each mass into moles

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Calculations in Chemistry

Calculations in Chemistry. To calculate the number of moles in a solid we use the following Mole Triangle. To calculate the number of moles in a solution we use the following Mole Triangle. g. n. c. v. n. gfm. n = number of moles c = concentatration (moles/litre)

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Molecular Formula

Molecular Formula. What is it?. Simplest formula just shows a ratio of atoms in a substance Simplest formula may or may not be the true molecular formula If you know the true mass of a substance, you can determine if the simplest formula is the molecular formula. Example 1.

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1) a) H = 2.06%, S = 32.69%, O = 65.25% b) Ca = 54.09%, O = 43.18%, H = 2.73% 2) 24 x .787 + 25 x .101 + 26 x .112 =

1 mol O 2. 2 mol MgO . x . x . 32.00 g O 2. 1 mol O 2. 40.31 g MgO. x . 1 mol MgO. 1) a) H = 2.06%, S = 32.69%, O = 65.25% b) Ca = 54.09%, O = 43.18%, H = 2.73% 2) 24 x .787 + 25 x .101 + 26 x .112 = 24.3 3) a) 98.08 g/mol, b) 759.70 g/mol

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Ulti Power Testo Boost Reviews, Cost, Price and Free Trial

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