OBJECTIVE 4:THE STUDENT WILL DEMONSTRATE AN UNDERSTANDING OF THE STRUCTURES AND PROPERTIESOF MATTER.

Basic Chemistry

Knows relationships exist between properties of matter and its components.

Properties of Matter

Mass The amount of stuff in an object. Measured in grams, g ; or kilograms, kg.

Volume The amount of space something takes

up. Measured in

If a solid: cubic meters, m3 ; cubic centimeters, cm3

If a liquid: liters, L ; milliliters; mL

Inertia A property of matter that resists a

change in motion. The bigger the mass, the more inertia it

has. The property of matter to keep doing

what it is doing.

Density Density is the state or quantity of being

dense; compactness; closely set together or crowded.

Density = mass per unit volume. Units: grams per cubic centimeter, g/cm3

; kilograms per cubic meter, kg/m3 ; grams per milliliter, g/mL; kilograms per liter, kg/L.

How much stuff is crammed into a volume. The density of water is 1 g/cm3

Investigate and identify properties of fluids including density, viscosity, and buoyancy; and

Relate the chemical behavior of an element including bonding, to its placement on the periodic table.

Atoms or Elements The atom is the basic unit of matter consisting

of a nucleus surrounded by electrons in discrete energy levels.

The nucleus is dense and contains protons and neutrons.

Protons are positively charged, electrons are negatively charged, and neutron have no charge (they are neutral).

The word atom is Greek and means uncuttable or indivisible, something that cannot be divided further.

These make up the Periodic Table.

Atomic Number The number of protons an atom has. It’s the identifying number that identifies

the element.8

OOxygen

15.9994

Atomic Number

Atomic Mass

Periodic Table

Periodic Table: Rows Rows are called periods. They are energy levels; Where the

electrons are. There are 7 periods (rows)

Periodic Table: Columns Columns are groups or families. They have similar chemical properties. They have the same number of valance

electrons. The last column (#18) are full and are

called the Nobel Gases or Inert gases.

Atomic Mass or Atomic Weight The number of protons plus the number

of neutrons in an element. Most elements can have different

numbers of neutrons so there can be different atomic masses for the same element. These are called isotopes.

The most abundant mass is what is reported on the periodic table.

Periodic Table: The Element

29

CuCopper63.546

Atomic numberNumber of

protonsIdentifies element

Name of element

Chemical Symbol

Atomic Mass (most abundant)

64 – 29 = 35 neutrons

Valance Electrons Electrons in the outer most energy level

of an atom. Valance electrons determine how the

atoms combine to make molecules. Rule of 8.

Ion An ion is an atom or molecule where the

total number of electrons is not equal to the total number of protons giving it a net positive or negative charge.

An ion is an atom that has too many or too few electrons (compared to its protons).

Molecule A molecule is two or more atoms

connected together by ionic or covalent bonds that make up a identifying substance.

The two atoms can be the same element. Diatomic molecules: O2; H2; N2

The molecule can be made of two or more different elements, Polyatomic: CO; NO; NaCl ; HCl ; CO2; H2O; C6H12O6 ; H2SO4

Reactants - Products In a chemical equation (formula) The reactants are what you start with.

They are on the left side of the equation. The products are what they (the

reactants) make. They are on the right side of the equation. The arrow points to the products.

Balancing a Chemical Equation Be able to balance a chemical equation. You must have the same number of

atoms (elements) on both sides of the You must have the same amount of mass

on both sides of the . Watch out for gas given off during a reaction.

Energy could be added or given off, but it should be equal as well.

Balance Chemical EquationsYou must be able to balance chemical equations. __Mg(s) + __O2(g) __MgO(s) __Fe(s) + __O2(g) __Fe2O3(s) __H2O(l) + __N2O3(g) __HNO2(aq) __Na2O(s) + __H20(l) __NaOH(aq) __Fe(s) + __H2O(l) __Fe3O4(s) + __H2(g)

Balanced equations Answers

2Mg(s) + 1O2(g) 2MgO(s)

4Fe(s) + 3O2(g) 2Fe2O3(s)

1H2O(l) + 1N2O3(g) 2HNO2(aq)

1Na2O(s) + 1H20(l) 2NaOH(aq)

3Fe(s) + 4H2O(l) 1Fe3O4(s) + 4H2(g)

Viscosity Viscosity is the internal friction of a fluid,

produced by the movement of its molecules against each other.

Viscosity causes the fluid to resist flowing.

The property of resistance of a fluid to flow.

The thickness of a fluid. Cold honey flows slower than water. Viscosity changes with temperature.

Buoyancy Buoyancy is the upward force that keeps

things afloat. When an object is placed in water, an object will float if its buoyancy is greater than its weight, and will sink if its weight is greater than its buoyancy.

The density of water is 1. Objects with a density less than 1 float, and greater than 1 sink.

Knows how solution chemistry is a part of everyday life.

Solutions

Dissolve To become absorbed in a liquid solution,

or make a solid do this. To fade away gradually and disappear or

make something do this. To break up into smaller or more basic

parts or make something do this.

Solvent A substance in which other substances

are dissolved, often a liquid. But not always.

Sugar dissolves in water. Sugar is the solute, water is the solvent.

CO2 is dissolved in soda pop. CO2 is the solute, soda pop is the solvent.

O2 is dissolved in water. O2 is the solute, water is the solvent.

Solute Solute is the stuff dissolved in the

solvent. Sugar dissolves in water. Sugar is the

solute, water is the solvent. CO2 is dissolved in soda pop. CO2 is the

solute, soda pop is the solvent. O2 is dissolved in water. O2 is the solute,

water is the solvent.

Solution In chemistry, a solution is a

homogeneous mixture composed of two or more substances. In such a mixture, a solute is dissolved in another substance, known as a solvent.

Usually the substance present in a greater amount is considered as the solvent. The solution that forms has the same physical state as the solvent.

Types of solutions

Liquids: Oxygen in

water CO2 in water Alcoholic

beverages Petroleum Sugar in water Body fluids

Solids: Steel Brass Alloys Polymers

Gas: Air

Homogeneous Homogeneous of the same kind. Having the same kind of constituent

elements, or being similar in nature. Having uniform composition. Being the same throughout. Smoooooth

Heterogeneous Heterogeneous consisting of dissimilar

parts. Consisting of parts that are unrelated or

unlike each other. Chunky

Electrolytic In chemistry, an electrolyte is any

substance containing free ions that makes the substance able to carry electricity (an electric current).

In most cases we are referring to a liquid, but it is not limited to liquids.

Knows that changes in matter affect everyday life.

Matter

Distinguish between physical and chemical changes in matter such as oxidation, digestion, changes in states, and stages in the rock cycle.

Investigate and identify the law of conservation of mass.

Phases of Matter: Physical Changes

increasing

temperature

Phase Changes of Water

Physical Change Change of phase: Solid , Liquid, Gas

from one to another. Phase change words: melt, freeze,

evaporate, condense, boil, sublime, deposit.

Mixtures and solutions are considered physical changes.

The substance keeps its chemical composition. Steam, water and ice are all forms of H2O.

Chemical Change Something new is made. Chemical composition is changed. Signs:

Color change Light or energy given off Fizzes or bubbles or gas forms Precipitate forms Gets hot or cold Makes an odor

Rusting is a chemical change. Souring milk is a chemical change. Cooking food is a chemical change. Food ripening or rotting is a chemical

change.

Melting ice is a physical change. Rocks breaking is a physical change. Crushing a tablet into tiny pieces is a

physical change.

Igneous Rocks Igneous rock (from the Latin ignis

meaning born of fire) is one of the three main rock types (the others being sedimentary and metamorphic rock).

Igneous rock is formed by magma (molten rock) cooling and becoming solid.

Sedimentary Rocks Sedimentary rock is formed by sedimentation of

material at the Earth's surface and within bodies of water.

Sedimentation is the collective name for processes that cause mineral and/or organic particles (detritus) to settle and accumulate or minerals to precipitate from a solution.

Particles that form a sedimentary rock by accumulating are called sediment. Before being deposited, sediment was formed by weathering and erosion in a source area, and then transported to the place of deposition by water, wind, mass movement or glaciers.

Metamorphic Rocks Metamorphic rock is the result of the

transformation of an existing rock type, the protolith, in a process called metamorphism, which means "change in form".

The protolith is subjected to heat and pressure causing profound physical and/or chemical change.

Metamorphic rocks are rocks that have "morphed" into another kind of rock.

Rock Cycle

Relate the structure of water to its function [as the universal solvent]

Relate the concentration of ions in a solution to physical and chemical properties such as pH, electrolytic behavior, and reactivity; and

Demonstrate how various factors influence solubility including temperature, pressure, and nature of the solute and solvent.

Polarity Polarity in chemistry is when a molecule

is arranged so that the molecule has a positive side (pole) and a negative side (pole). The molecule acts like a magnet due to the arrangement of its composing atoms.

Water is a polar molecule. Water is called the “Universal Solvent”

because of its molecular make up.

Water is Polar. H2O

pH pH is used to measure acidity(H+) and basicity

(OH−) It measures the concentration of dissolved

hydrogen ions. Acids are from 1 to 7, bases are from 7 to 14; 7

being neutral. The farther from 7 the stronger the acid/base.

Acids turns litmus paper red, bases turn it blue.

1 2 3 4 5 6 7 8 9 10 11 12 13 14

http://upload.wikimedia.org/wikipedia/commons/4/46/PH_scale.png

Solubility factors Making the solute smaller in size

increases solubility. Heating the solution increases the

solubility. Stirring the solution increases the

solubility. Increasing the solvent, or reducing the

solvent increases the rate of solubility. Pressure has an affect on solubility.

Conservation of Mass The total mass before equals the total

mass after. Mass cannot be created or destroyed. The same number of atoms must be on

both sides of a chemical equation.

Conservation of Energy The total energy before equals the total

energy after. Energy can change forms. Work is a form of energy. In a chemical equation, energy can be

added to or released from a chemical reaction, but you must be able to account for it.

Must Knows There will be several questions involving density. Be able to use the density equation. Water has a density of 1 gm/ml. Object’s with a

density greater than 1, sink in water and object’s with a density less than 1 float in water. Watch out for floater – sinker questions in other materials.

They like layer problems. Top layers are less dense than lower layers.

The periodic table: Rows are periods and show energy (electron) levels; Columns are groups or families and have similar chemical properties and the same number of valance electrons.

Must Knows, page 2 Know pH. 7 is neutral (pure water) and the farther you

go from 7 the stronger the substance: 1very strong acid; 14 very strong base. Stomach acid is very strong acid. Bleach is a very strong base.

Chemical and physical changes. Electrolytic means it carries electricity easily. Know safety warning signs and procedures. Know the periodic table, valance numbers, elements

with like chemical properties, and energy levels. Know how to find the number of protons, neutrons, and

electrons. Know what elements are attracted to others. Know what electrolytic means.

Must Know page 3 Metals, non-metals, and metalloids. The dividing line between metals and

non-metals. Noble gases. (Inert) Valance electrons. Viscosity Density