Find your seats and take out your notebook. Agenda for Tuesday March 22 nd 1.Matter and Mixtures Notes

Another resource

Composition of Matter Matter – anything that has mass and takes up space Element – substance that cannot be separated or broken down into simpler substances Atom – smallest unit of an element that maintains the properties of that element

Compounds Compound – substance with 2 or more different atoms (elements) Molecules – smallest unit of a compound that still maintains the properties of the compound Chemical Formulas

Mixtures Pure substances – only 1 element or compound Mixture – combination of 2 or more substances – Homogenous – contains substances blended evenly throughout – Heterogeneous – a mixture of different substances that can easily be distinguished from each other

Homogenous Mixtures Solution – homogenous mixtures – small particles, cannot be seen with a microscope – Particles do not settle to the bottom Examples – Salt water – Sugar water

Heterogeneous Mixtures Suspensions - visible particles will settle – Muddy water

Heterogeneous Mixtures Colloid = suspension where particles will not settle out of the mixture on their own – Milk, fog, smoke, gelatin desserts – Tyndall effect – scattering of light by larger particles Emulsion – two immiscible (unblendable) liquids mix together – mayonnaise

Predicting Types of Mixtures 1 substance 2 Substances Pure Substance Mixture Separates easily/ on its own Suspension No visible particles, Looks uniform throughout Won’t separate by physical means Solution Visible particles/cloudy Colloid Won’t separate on its own/cloudy Heterogeneous mixture Homogeneous Mixture

Homework Questions 1 – 8 page 44 Questions 1-3, 7 on page 231

Define homogeneous and heterogeneous mixtures. Agenda for Wednesday March 23 rd 1.Mixture lab

What is the difference between a compound and an element? Agenda for Thursday March 24 th 1.Solubility Notes 2.Solubility Lab

Key Terms Solute – stuff we want to dissolve Solvent – substance in which we dissolve something Solubility – maximum amount of solute that can dissolve in a solvent – Different for different substances – Depends on pressure & temp

Concentration Concentration – amount of a solute dissolved in a given volume of solution – A lot of solute is called concentrated – Little solute is called dilute

Saturation Saturated – a solution that can dissolve no more solute – Excess solute visible Unsaturated – can dissolve more solute Supersaturated – holds more solute than it normally can

Kool – Aid Lab

Define Solvent and Solute Agenda for Friday March 25 th 1.Quiz 2.Solubility of Salt lab 3.Concept Review

List 2 factors that affect solubility. Agenda for Monday March 28 th 1.Salt Lab 2.Physical/Chemical Properties 1.Demos

What is the common name for sodium chloride? Agenda for Tuesday March 29 th 1.Finish Lab 2.Physical/Chemical Changes

Properties of Matter Physical – characteristic of a material you can manipulate without changing the identity of a substance – shape, size, density, melting point, boiling point, color Physical Change - a change in size, shape or state of matter – dissolving

Properties of Matter Chemical - characteristic of a substance that indicates whether it can undergo a certain chemical change – New substances produced – Reactivity, flammability (ability to burn) Chemical Change - change of one substance to another – accompanied by heat, light, color, and sound

States of Matter Kinetic Theory – All matter is made of atoms and molecules – These particles are always in motion. Higher temp = faster movement – At same temp., heavier molecules move slower 3 different states of matter – Solid, liquid, gas