Understanding Elements, Compounds, and Mixtures: Exploring Properties of Solutions
Today’s agenda focuses on distinguishing among elements, compounds, and mixtures. We will explore the periodic table, understand how to form compounds by bonding elements, and differentiate between homogeneous and heterogeneous mixtures. Additionally, we will identify properties of solutions, including solute and solvent in different states (solid, liquid, gas), and learn procedures to determine solution concentrations in ppm, ppb, and molarity. Practice test exercises will reinforce these concepts through real-world examples.
Understanding Elements, Compounds, and Mixtures: Exploring Properties of Solutions
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Presentation Transcript
Catalyst Calculators and periodic tables today!
Objective • Performance Indicator: Distinguish among elements, compounds, and mixtures. • Practice test #25
Elements and Compounds • Where do you find all the elements? • Periodic table • What do you have to do to form a compound? • Bond together two or more elements
Mixtures • A mixture is a mix of elements, compounds, or both that are not chemically bonded together • Homogeneous vs. heterogeneous?
Objective • Performance Indicator: Identify properties of a solution: solute and solvent in a solid, liquid or gaseous solution: procedure to make or determine the concentration of a solution in units of ppm, ppb, molarity, percent composition, factors that affect the rate of solution. • Practice test #26-29
MOLARITY M= Moles of solute Liters of solution Change mL to L by moving the decimal point three times! Concentration is commonly measured by chemists using Molarity: the number of moles of solute per liter of solution
EXAMPLES • Suppose that 0.30 mol KBr are present in 0.40L of solution. What is the molarity of the solution? • Ms. Myers makes 7.5 L of a 6 M NaOH solution. How many moles of NaOH did she use? • How many grams of BeCl2 would be needed to make 1 L of a 5.0 M BeCl2 solution? • Why is grams underlined?
