The Nature of Matter What is matter Matter

  • Slides: 64
Download presentation
The Nature of Matter

The Nature of Matter

What is matter? Matter: Anything that has mass and volume Matter can be measured

What is matter? Matter: Anything that has mass and volume Matter can be measured in these ways: • Volume: amount of space that matter takes up • Mass: a measure of matter’s inertia (more mass = greater inertia) -mass is always constant, no matter where the object is in the universe; weight is a measure of the force of gravity. • Density: the mass of a given volume of a substance • Length: You hopefully know what this is…

Physical properties of matter: Physical Property: Things that can be observed about a substance

Physical properties of matter: Physical Property: Things that can be observed about a substance or object without changing the identity of the substance or object. Examples of Physical Properties: • Color • Odor • Mass • Volume • How well it conducts electricity • Malleablity (ability to be bent into shapes) • • Density ( d = m/v) State at room temperature Heat or electricial conductivity Ductility (ability to be pulled in wire)

Characteristic property: a property of a substance that can help identify a substance. Examples:

Characteristic property: a property of a substance that can help identify a substance. Examples: • Copper has a reddish color • Water has a density of 1 g/ml • Diamonds are much harder than other minerals.

Physical & Chemical Changes: Physical Change: a change in a substance that does not

Physical & Chemical Changes: Physical Change: a change in a substance that does not change the identity of a substance. (example: crumpling up a piece of paper. ) Chemical change: a change in a substance that changes its identity (examples: setting a piece of paper on fire; iron rusting in salt water. )

Chemical Properties: Chemical properties describe matter’s ability to turn into other types of matter.

Chemical Properties: Chemical properties describe matter’s ability to turn into other types of matter. Examples: • Flammability: the ability to burn (be converted to energy) • Reactivity: the ability to combine with other types of matter and become a new substance

LO: Describe the physical and chemical properties of matter. SLE: Meet or exceed NGSS.

LO: Describe the physical and chemical properties of matter. SLE: Meet or exceed NGSS. Questions from properties of matter notes: 1. ) List three examples of physical properties. 2. ) What is a characteristic property of matter (define the term)? 3. ) Can the mass of an object be used as a characteristic property? Why or why not? 4. ) What physical properties (besides mass) can be considered characteristic properties? 5. ) What’s the difference between a physical property and a chemical property?

LO: Describe physical properties of matter SLE: Meet or exceed NGSS Questions from Science.

LO: Describe physical properties of matter SLE: Meet or exceed NGSS Questions from Science. Saurus, p. 250 -254: 1. ) Define these words: Malleability, ductility, conductivity, solubility 2. ) Describe the differences between a physical and a chemical change. 3. ) Describe what the atoms (particles) of a substance are doing in solid, liquid, and gaseous states of matter.

LO: Describe properties of matter SLE: Meet or exceed NGSS Checkpoint Quiz on the

LO: Describe properties of matter SLE: Meet or exceed NGSS Checkpoint Quiz on the Properties of Matter: 1. ) What is matter? 2. ) What are physical properties of matter? 3. ) What is a characteristic property? 4. ) Give an example of a physical change. 5. ) Give an example of a chemical change.

LO: Identify a substance using characteristic properties of matter SLE: Work collaboratively Question: What

LO: Identify a substance using characteristic properties of matter SLE: Work collaboratively Question: What metals are these bolts made from? Directions: 1. Observe the bolts that are provided to you. 2. Find their mass, volume and density. 3. Compare your density to the published densities of metal, and decide what metal it is. Mass (g): Volume (ml: Density (g/ml): The bolt is made from: ________

LO: Identify and describe historical models of the atom SLE: Meet or exceed NGSS

LO: Identify and describe historical models of the atom SLE: Meet or exceed NGSS Review Questions on Models of the Atom: 1. What did Democritus think of the structure of matter? 2. Discuss four ideas Dalton had about atoms. 3. What did Thomson discover about atoms? 4. How did Rutherford’s model of the atom differ from Thomson’s model? 5. How did Bohr Modify Rutherford’s model?

LO: Describe how models of the atom have changed over time. SLE: Meet or

LO: Describe how models of the atom have changed over time. SLE: Meet or exceed NGSS Checkpoint Quiz on Historical Models of the Atom: 1. Who first suggested that matter is made of atoms? 2. List two inferences that Dalton made about atoms. 3. Draw and label a diagram of Thomson’s model of the atom. 4. Draw and label a diagram of Rutherford’s model of the atom. 5. What modification did Bohr make to Rutherford’s model?

Signs of chemical change: • • Change in color Change in odor Forms a

Signs of chemical change: • • Change in color Change in odor Forms a precipitate Creation of gas (fizzing, bubbling) Production of heat or other change in temperature Creation of light Creation of sound (e. g. , explosion) The most important sign that a chemical change has occurred is that it cannot be easily reversed.

Elements vs. Compounds: Element: A substance which contains only identical atoms. Examples: hydrogen, helium,

Elements vs. Compounds: Element: A substance which contains only identical atoms. Examples: hydrogen, helium, oxygen Molecule: A group of atoms that are connected (either by sharing or transferring electrons) Compound: A substance that contains two or more types of atoms that are chemically bonded together. Examples: water, carbon dioxide

How to Read the Periodic Table:

How to Read the Periodic Table:

LO: Describe the behavior of particles in matter during changes of state. SLE: Meet

LO: Describe the behavior of particles in matter during changes of state. SLE: Meet or exceed NGSS Checkpoint Quiz on Particle Motion During Changes of State: 1. Describe the particle model of matter. 2. Generally speaking, what happens to the motion of particles in matter when the temperature increases? 3. What happens to the volume of a gas when the temperature decreases? 4. Describe Boyle’s law. 5. Describe what happens to water particles when you freeze water.

Isotopes of Atoms: Isotope: the number of neutrons varies from the most-common variety listed

Isotopes of Atoms: Isotope: the number of neutrons varies from the most-common variety listed in the periodic table. Example: Most atoms of carbon have 6 neutrons. However, some carbon atoms may have more or less than this number. Therefore, their mass may be more or less than the usual 12 AMU (atomic mass units)

Naming Isotopes: Isotopes of a given element are named (numbered) according to their mass

Naming Isotopes: Isotopes of a given element are named (numbered) according to their mass number. Example: a carbon atom that has 6 protons and 8 neutrons has a mass of 14, so the name of that isotope is C-14.

Properties of isotopes: • Generally, isotopes of an element have the same physical and

Properties of isotopes: • Generally, isotopes of an element have the same physical and chemical properties of other isotopes of the same element. • However, some isotopes have unstable nucleii, and they decay rapidly (i. e, are radioactive. ) For example C-14 is somewhat radioactive

Forces Within atoms (and throughout the universe): • Gravity: exists because mass curves space-time

Forces Within atoms (and throughout the universe): • Gravity: exists because mass curves space-time • Electromagnetic force: the force created by particles with positive or negative electric charges • Strong nuclear force: the force that keeps particles in the atom from flying apart from one another • Weak nuclear force: The force that allows subatomic particles to turn into other types of particles (and is the cause of radioactive decay)

Organization of the Periodic Table: Elements, when arranged by atomic number (or even by

Organization of the Periodic Table: Elements, when arranged by atomic number (or even by atomic mass), follow a pattern known as the Periodic Law: The physical and chemical properties of the elements re-occur in a regular pattern as you go through the elements in order of their atomic numbers.

Groups and Periods: The periodic table is organized into groups and periods: Groups (columns)

Groups and Periods: The periodic table is organized into groups and periods: Groups (columns) have similar properties. Periods (rows) have similar atomic numbers and masses.

Main Regions of the Periodic Table: 1. Metals: Most elements are metals. They are

Main Regions of the Periodic Table: 1. Metals: Most elements are metals. They are mainly listed to the left of the zigzag line (commonly called the staircase). Most metals are: • Solid at 20 o C • Shiny • Ductile • Malleable • Good conductors of heat and electricity

2. Nonmetals: Nonmetals are mostly to the right of the staircase. Most nonmetals: •

2. Nonmetals: Nonmetals are mostly to the right of the staircase. Most nonmetals: • Are gases or solids at 20 o C • Have almost completely full outer electron orbits • Are poor conductors • Are brittle (if solid)

3. Metalloids: metalloids are found on the staircase. They have some properties of metals,

3. Metalloids: metalloids are found on the staircase. They have some properties of metals, and some properties of nonmetals.

A More Detailed Look at the Table:

A More Detailed Look at the Table:

Properties of the Groups: Group 1: Alkali Metals: They are highly reactive, soft, and

Properties of the Groups: Group 1: Alkali Metals: They are highly reactive, soft, and brittle. They all have one electron in their outer orbit. Group 2: Alkaline Earth Metals: They are like group 1, but slightly less reactive. They have 2 electrons in their outer orbit. Groups 3 -12: Transition Metals: Have “normal” properties of metals. They are less reactive than groups 1 -2. Electrons flow freely among atoms (which is why they’re good conductors)

Group 17: Halogens. Very reactive nonmetals. They frequently form chemical bonds with metals in

Group 17: Halogens. Very reactive nonmetals. They frequently form chemical bonds with metals in groups 1 and 2. Group 18: Noble Gases. These gases have completely full outer electron orbits, so do not form bonds with any other elements. They are always found in pure form in nature.

LO: Describe the organization of the periodic table SLE: Meet or exceed NGSS Checkpoint

LO: Describe the organization of the periodic table SLE: Meet or exceed NGSS Checkpoint Quiz on the Periodic Table: 1. Why is it called the periodic table? 2. Which group in the periodic table consists of highly reactive metals? (Write either the name or number of the group) 3. Which group in the periodic table consists of highly reactive nonmetals? 4. Which group in the periodic table consists of elements that don’t react with any other elements at all? 5. Nitrogen has an atomic number of 7 and an atomic mass of 14. 01 AMU. Draw a Bohr diagram of an atom of this element.

States of matter and the particle model: Three states of matter: 1. Solids: have

States of matter and the particle model: Three states of matter: 1. Solids: have a definite shape and volume. Particles within solids are vibrating, but not moving much in relation to each other. Types of solids: • Crystalline: particle arrangement is very orderly, and follows a definite pattern. • Amorphous: particle arrangement is random

2. Liquids: liquids have a definite volume, but they take the shape of the

2. Liquids: liquids have a definite volume, but they take the shape of the container they are in. Particles in a liquid move around quite a bit, but their energy level (and velocity) is relatively low.

3. Gases: Gases have no definite shape or volume. The particles have a lot

3. Gases: Gases have no definite shape or volume. The particles have a lot of energy and are moving very fast, and will rapidly spread out to fill whatever space they are in. The space between gas molecules is very large compared to solids and liquids.

Two Gas Laws: 1. Charles’ Law: Given the same amount of pressure, if you

Two Gas Laws: 1. Charles’ Law: Given the same amount of pressure, if you increase the temperature of a gas, the volume will also increase.

Boyle’s Law: Given the same temperature, if you increase the pressure on a gas,

Boyle’s Law: Given the same temperature, if you increase the pressure on a gas, the volume will decrease.

Homework: LO: Describe states of matter in terms of the particle model of matter.

Homework: LO: Describe states of matter in terms of the particle model of matter. SLE: Meet or exceed NGSS. 1. Read p. 36 -45 2. Review questions p. 39, 45

LO: Describe endothermic and exothermic reactions. SLE: Work cooperatively. Reaction 1: • • 1.

LO: Describe endothermic and exothermic reactions. SLE: Work cooperatively. Reaction 1: • • 1. Place thermometer in jar and close lid. • 2. Wait 5 minutes and record temperature. • 3. Soak steel wool in vinegar for 5 minutes. • 4. Wrap vinegar-soaked steel wool around thermometer bulb, place back in jar. • 5. After 5 more minutes, record temperature again. • • Temperature before vinegar: ______C • • Temperature after vinegar: _____C • • What happened? Why? Reaction 2: 1. Pour some vinegar (citric acid) into a beaker. 2. Record temperature. 3. Stir in some baking soda. 4. Wait 30 -60 seconds 5. Record temperature again. Temperature before Sodium bicarbonate: ______C Temperature after Sodium bicarbonate: _______C What happened? Why? In general, what is the difference between exothermic and endothermic reactions?

LO: Describe the crystal structure of some solids SLE: Work cooperatively Salt crystal shape:

LO: Describe the crystal structure of some solids SLE: Work cooperatively Salt crystal shape: Sugar crystal shape:

LO: Describe states of matter SLE: Apply academic habits for success Checkpoint quiz on

LO: Describe states of matter SLE: Apply academic habits for success Checkpoint quiz on states of matter: 1. Describe the motion of particles in solids, liquids and gases. (2 pts) 2. State Charles’ Law. 3. State Boyle’s Law. 4. If you decrease the pressure applied to a certain volume of gas, what will happen to the volume? Why?

Compounds and Chemical Bonds: Review: An element is a substance that contains only a

Compounds and Chemical Bonds: Review: An element is a substance that contains only a single type of atom. A compound is a substance that contains molecules that are composed of two or more different kinds of atoms. A molecule is a collection of two or more atoms that are bonded together through the transfer or sharing of electrons.

Types of chemical (molecular) bonds: 1. Ionic Bond: created when an electron in the

Types of chemical (molecular) bonds: 1. Ionic Bond: created when an electron in the outer orbit of one atom gets transferred to another atom. This transfer creates two ions (atoms with positive or negative charge) , one of which is positively charged, and one of which is negatively charged. They then bond together via electromagnetic attraction.

2. Covalent Bonds: are formed when two or more atoms share electrons in their

2. Covalent Bonds: are formed when two or more atoms share electrons in their outer (valence) orbit. Diatomic molecules (O 2 for example) are formed by covalent bonds.

Homework: LO: Describe kinds of chemical bonds SLE: Work independently 1. Read p. 8

Homework: LO: Describe kinds of chemical bonds SLE: Work independently 1. Read p. 8 -17 in Interactions of Matter 2. Review questions on p. 11 & 17

LO: Compare strength of covalent and ionic bonds. SLE: Work collaboratively Problem: Are ionic

LO: Compare strength of covalent and ionic bonds. SLE: Work collaboratively Problem: Are ionic bonds harder to break apart than covalent bonds? Hypothesis: Independent variable: Dependent variable: 3 Controls: Procedure: 1. Put salt (ionic bond, Na. Cl) in a pan 2. Place pan on a hot plate and heat on high for 5 -10 minutes. 3. Repeat steps #1 -2 with sugar (Covalent bond, C 6 H 12 O 6). 4. Observe and record results. Observations: What happened when salt was heated: What happened when sugar was heated: Conclusion:

LO: Describe how elements are chemically combined SLE: Meet or exceed NGSS Checkpoint Quiz

LO: Describe how elements are chemically combined SLE: Meet or exceed NGSS Checkpoint Quiz on Chemical Bonds #2: 1. Describe how covalent bonds happen. 2. Describe how ionic bonds happen. 3. Write the formula for carbon tetrahydride. 4. Write the formula for potassium chloride. 5. Write the formula for aluminum oxide.

Law of Conservation of Mass: In any physical system, even during a chemical reaction,

Law of Conservation of Mass: In any physical system, even during a chemical reaction, the total amount of mass (i. e. , the total number of atoms) will not change.

LO: Model the law of conservation of mass. SLE: Work collaboratively. Problem: If a

LO: Model the law of conservation of mass. SLE: Work collaboratively. Problem: If a gas is produced in a closed system during a chemical reaction, does the total mass of the system stay the same? Hypothesis: Independent variable: Dependent variable: 3 Controls: Procedure: 1. Fill one Dixie cup halfway full of baking soda and another Dixie cup halfway full of vinegar. 2. Put both cups in a large Ziplock bag; be careful not to spill the contents of the cups! 3. Measure the total mass of the ziplock bag with the two cups. 4. Seal the ziplock bag shut and mix the contents of the cups. (In that order) 5. After 2 minutes, find the mass of the bag and cups again. 6. Repeat Steps 1 -4, but mix the contents of the cups without sealing the Ziplock bag. Data: Type of system: Mass before Mass after reaction (g): Closed Open Conclusion:

Forming New Substances: Chemical Reaction: A process in which one or more substances is

Forming New Substances: Chemical Reaction: A process in which one or more substances is changed into one or more new substances with different properties. Reactants: the substances you start out with. Products: the substances you end up with.

Signs of chemical reactions: • • • Formation of a gas. Formation of a

Signs of chemical reactions: • • • Formation of a gas. Formation of a new solid (precipitate) Change in temperature Change of color Creation of light

Chemical Formulas: Chemical formula: a formula that tells you what molecules of a compound

Chemical Formulas: Chemical formula: a formula that tells you what molecules of a compound look like: HCl: Hydrogen chloride; 1 atom of hydrogen, 1 atom of chlorine in each molecule. H 2 SO 4: Hydrogen sulfate; 2 atoms of hydrogen, 1 atom of sulfur, and 4 atoms of oxygen.

Predicting chemical formulas: The formula for covalent compounds is just based on the name:

Predicting chemical formulas: The formula for covalent compounds is just based on the name: Carbon disulfide: 1 C, 2 S, so it’s CS 2 Carbon monoxide: 1 C, 1 O, so it’s CO

For ionic compounds, you have to know the group numbers and charges of the

For ionic compounds, you have to know the group numbers and charges of the ions: Magnesium Chloride: Mg is in group 2 and has a charge of +2; Cl is in group 17, has room for 1 extra electron, so has a charge of -1: But Mg wants to give 2 electrons away, so 2 Cl atoms are involved in the bond: Mg. Cl 2

Charges of polyatomic ions: • • • Ammonium ion, NH 4; 1+ Carbonate ion,

Charges of polyatomic ions: • • • Ammonium ion, NH 4; 1+ Carbonate ion, CO 3; 2− Hydroxide ion, OH; 1− Nitrate ion, NO 3; 1− Phosphate ion, PO 4; 3− Sulfate ion, SO 4; 2− Unfortunately, because polyatomic ions involve reactions with molecules that are based on covalent bonds, these need to just be remembered or looked up.

LO: Write chemical formulas SLE: Meet or exceed NGSS Checkpoint Quiz on Chemical Formulas:

LO: Write chemical formulas SLE: Meet or exceed NGSS Checkpoint Quiz on Chemical Formulas: Write the name of the compound: 1. KCl 2. Al 2 O 3 Write the formula: 3. Sodium hydroxide 4. Calcium oxide 5. Magnesium chloride

Chemical Equations: Chemical Equation: a way to describe what happens in a chemical reaction

Chemical Equations: Chemical Equation: a way to describe what happens in a chemical reaction by displaying the changed chemical formulas of the substances involved. Reactant Product

Balancing Chemical Equations: It’s really important that chemical equations: 1. Reflect reality; 2. Reflect

Balancing Chemical Equations: It’s really important that chemical equations: 1. Reflect reality; 2. Reflect (obey) the law of conservation of mass. C + O 2 CO 2

To balance equations, because of the way electrons move around in chemical bonds, coefficients

To balance equations, because of the way electrons move around in chemical bonds, coefficients must be added to the equation: H 2 + O 2 H 2 O : Not balanced 2 H 2 + O 2 2 H 2 O Balanced

Homework: LO: Describe chemical reactions using chemical equations. SLE: Work independently. 1. Read pages

Homework: LO: Describe chemical reactions using chemical equations. SLE: Work independently. 1. Read pages 28 -37 in Interactons of Matter. 2. Complete review questions on p. 37 (on loose leaf).

Types of Chemical Reactions: Synthesis Reaction: Two substances combine to form one compound: 2

Types of Chemical Reactions: Synthesis Reaction: Two substances combine to form one compound: 2 Na + Cl 2 2 Na. Cl Decomposition Reaction: A single compound breaks down and forms two or more simpler substances: 2 H 2 O 2 H 2 + O 2

Single-Replacement Reaction: One or more elements replaces an element in a compound: Zn +

Single-Replacement Reaction: One or more elements replaces an element in a compound: Zn + 2 HCl Zn. Cl 2 + H 2 Double-Replacement Reaction: elements in two different compounds change places: Na. OH + KCl Na. Cl + KOH

Homework: LO: Identify and describe types of chemical reactions SLE: Work independently 1. Read

Homework: LO: Identify and describe types of chemical reactions SLE: Work independently 1. Read p. 38 -48 2. Review questions p. 50 -51 all

LO: Describe chemical compounds SLE: Meet or exceed NGSS Checkpoint Quiz on Chemical Compounds:

LO: Describe chemical compounds SLE: Meet or exceed NGSS Checkpoint Quiz on Chemical Compounds: 1. Describe what conservation of mass means. Name these compounds: 2. Cu. Cl 3. K 3 PO 4 Write the formula for these compounds: 4. Sodium chloride 5. Aluminum bromide

LO: Balance chemical equations SLE: Meet or exceed NGSS Checkpoint Quiz: Balancing Chemical Equations

LO: Balance chemical equations SLE: Meet or exceed NGSS Checkpoint Quiz: Balancing Chemical Equations 1. Na. Br + Ag 2 SO 4 Na 2 SO 4 + Ag. Br 2. Pb. O 2 Pb. O + O 2 3. KI + Cl 2 KCl + I 2 4. H 2 O 2 H 2 O + O 2 5. H 2 O + CO 2 C 6 H 12 O 6 + O 2

LO: Describe the creation and use of synthetic materials SLE: Work collaboratively How to

LO: Describe the creation and use of synthetic materials SLE: Work collaboratively How to Make a “natural” (vs. totally synthetic) plastic: 1. Heat up a pan (about 1 cup) of milk until it simmers. 2. As it simmers, stir in 1 spoonful of vinegar 3. Continue adding spoonfuls of vinegar until it begins to jell. 4. Allow the mixture to cool. 5. Wash the rubbery material off with water. 6. Observe your plastic, and make note of its properties.