Introduction to Matter Ms Ho DO NOW Based

Introduction to Matter Ms. Ho

DO NOW Based on your current understanding of MATTER, draw a star next to any example below that is considered MATTER. ______your laptop ______sound ______a piece of gold ______a cell ______light ______bacteria ______air ______an atom

Agenda • • Notes on Matter Assign Homework Practice Questions Ticket to Leave

What Properties Describe Matter? • Matter is anything that has mass and takes up space. • All the “stuff” in the natural world is matter. • Matter can have many different properties, or characteristics that are used to describe, identify, and classify it. • Matter can be hard or soft, hot or cold, liquid, solid, or gas. • Some matter catch fire easily while others do not burn. • Chemistry is the study of matter and how it changes. Substances are one type of matter.

Substances • A substance is a single kind of matter that is pure, meaning it has a specific composition. • That composition gives it specific properties. • Every form of matter has two kinds of properties—physical properties and chemical properties.

Physical Property • A physical property is a characteristic of a substance that can be observed without changing it into a different substance. • Examples of physical properties include: a. state of matter b. freezing point c. melting point d. boiling point e. luster f. flexibility g. ability to conduct heat and an electric current h. hardness i. temperature j. texture k. color

Chemical Properties • A chemical property is an ability to change into different substances. • In order to observe the chemical properties of a substance, the substance must be changed into a different substance. • Examples of chemical properties include a. rusting b. tarnishing c. flammability

Practice Questions (page 6 -7)

DO NOW Please complete assignment 8. S. 3. A as your DO NOW.

Practice Questions Continued

OBJECTIVE: SWBAT classify matter. ? ?

OBJECTIVE: SWBAT classify matter. Matter ? ? ?

CTIVE: SWBAT classify matter. Matter: Anything that has mass (consists of atoms) and has volume (occupies space).

OBJECTIVE: SWBAT classify matter. Matter Pure Substance ? ? ?

CTIVE: SWBAT classify matter. Pure Substance: A sample of matter that consists of only one component with definite physical and chemical properties and a definite composition. Table salt Pure silver

OBJECTIVE: SWBAT classify matter. Matter Pure Substance ? Mixture ? ? ?

CTIVE: SWBAT classify matter. Mixture: A sample of matter composed of two or more pure substances, but each keeps its original properties. Chocolatechip cookies Fruit punc

OBJECTIVE: SWBAT classify matter. Matter Pure Substance Elements Mixture ? ? ?

CTIVE: SWBAT classify matter. Element: A pure substance that cannot be broken down into simpler substances. Pure copper Pure calcium

OBJECTIVE: SWBAT classify matter. Matter Pure Substance Element Compound Mixture ? ?

CTIVE: SWBAT classify matter. Compound: A substance formed by the chemical combination of two or more elements.

OBJECTIVE: SWBAT classify matter. Matter Pure Substance Element Mixture Compound Homogeneous

CTIVE: SWBAT classify matter. Homogeneous: A mixture has the same uniform appearance and composition throughout.

OBJECTIVE: SWBAT classify matter. Matter Pure Substance Element Mixture Compound Homogeneous Heterogeneous

CTIVE: SWBAT classify matter. Heterogeneous: A mixture that consists of visibly different substances or phases.

DO NOW

Atoms • According to the particle theory, all matter is made up of atoms. • An atom is the basic particle from which all elements are made. • An atom has a positively charged center, or nucleus, surrounded by a negatively charged “cloud. ” • Atoms of most elements can combine with other atoms by forming chemical bonds.

Chemical Bonds • A chemical bond is a force of attraction between two atoms. • The result of a chemical bond is often a molecule, or a group of two or more atoms held together by chemical bonds. • A molecule can be made of atoms of different elements or atoms of the same element.

Atoms and Molecules are made up of groups of atoms. How many atoms are in each of these molecules?

Mass and Volume • Weight is a measure of the force of gravity on an object. Weight varies with location in the solar system. • A more massive object will exert a greater gravitational force, so the weight of an object on that more massive planet or moon will be greater. • Weight is measured with a scale. • Mass is the amount of matter in an object. It does not change with location. Mass is constant. For this reason, scientists prefer to describe matter in terms of mass rather than weight.

Units of Measurement • • • To measure the properties of matter, scientists use the International System of Units, or SI. The SI unit of mass is the kilogram (kg). If a smaller unit of mass is needed, the gram (g) is used. There are 1, 000 grams in a kilogram or 0. 001 kilogram in a gram. The first country to use an SI-based system of measurement was France in 1795. Today, there are only three countries in the world who have not adopted the SI system—Liberia, Myanmar, and the United States.

Volume

Density

Density • The density of water is 1 g/m. L, or 1 g/cm³. • Objects with greater densities will sink. • Objects with lesser densities will float. • Density is a physical property of a substance. • It can be used to identify an unknown substance.

Common Objects in Nanometers (nm)

Compounds From Elements What are the properties of copper, sulfur, and copper sulfide?

Mixtures Which of these foods are heterogeneous and which are homogeneous?

Separating Mixtures Which type of separation method is used in each of these situations?

Measuring Weight Use the weight of the first scale to estimate the weight of the fish on the other scales.

Measuring Mass What is the mass of each object, measured in kilograms?

Calculating Volume What is the volume of the suitcase?

Measuring Irregular Objects One way to measure the volume of an irregular object is to submerge it in liquid in a graduated cylinder.

Density Liquids can form layers based on density. Which colored layer of liquid represents Water: 1. g/ml, Honey: 1. 36 g/ml, Dish Soap: 1. 03 g/ml, Corn Syrup: 1. 33 g/ml, Vegetable oil: 0. 91 g/ml?

Examples of Chemical Change

Conservation of Mass Count the atoms of each element before and after the chemical change.

Temperature of Two Reactions What are the changes in temperatures for each reaction during the ten minutes?

Indiana Jane and the Investigation of Matter Indiana Jane is hunting for lost treasures of matter. Broken clay pot Field notes: I’ve come across some clay pots. Many have been broken or cracked over time. —IJ Yellowed, torn map Field notes: The paper of this ancient map has suffered from changes over the years making it nearly impossible to read. —IJ