Basic Chemistry

1. Objective 4:The student will demonstrate an understanding of the structures and propertiesof matter. Basic Chemistry

2. Properties of Matter Knows relationships exist between properties of matter and its components.

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

4. 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

5. 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.

6. 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

7. 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.

8. 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.

9. Atomic Number • The number of protons an atom has. • It’s the identifying number that identifies the element. Atomic Number 8 O Oxygen 15.9994 Atomic Mass

10. Periodic Table

11. Periodic Table: Rows • Rows are called periods. • They are energy levels; Where the electrons are. • There are 7 periods (rows)

12. 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.

13. 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.

14. Periodic Table: The Element Atomic number Number of protons Identifies element 29 Cu Copper 63.546 Chemical Symbol Name of element Atomic Mass (most abundant) 64 – 29 = 35 neutrons

15. 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.

16. 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).

17. 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

18. 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.

19. 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.

20. Balance Chemical Equations You 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)

21. 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)

22. 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.

23. 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.

24. Solutions Knows how solution chemistry is a part of everyday life.

25. 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.

26. 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.

27. 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.

28. 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.

29. Types of solutions • Solids: • Steel • Brass • Alloys • Polymers • Gas: • Air • Liquids: • Oxygen in water • CO2 in water • Alcoholic beverages • Petroleum • Sugar in water • Body fluids

30. 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

31. Heterogeneous • Heterogeneous consisting of dissimilar parts. • Consisting of parts that are unrelated or unlike each other. • Chunky

32. 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.

33. Matter Knows that changes in matter affect everyday life.

34. 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.

35. Phases of Matter: Physical Changes increasing temperature

36. Phase Changes of Water

37. 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 keepsits chemical composition. Steam, water and ice are all forms of H2O.

38. 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

39. 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.

40. 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.

41. 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.

42. 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.

43. Rock Cycle

44. 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.

45. 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.

46. Water is Polar. • H2O

47. 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

49. 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.

50. 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.