TAKS Vocabulary

1. TAKS Vocabulary

2. Scientific Method

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. 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.

8. 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.

9. Chemistry

10. Periodic Table

11. 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.

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

13. 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

14. 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.

15. Water is Polar. • H2O

16. 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.

17. 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.

18. 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.

19. 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.

20. 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

21. 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

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

23. 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.

24. 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

25. 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

26. 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.

27. 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.

28. 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

29. 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.

30. 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).

31. 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.

32. 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

34. 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.

35. Physics

36. Newton’s First law of Motion • An object in motion will stay in motion and an object at rest will stay at rest unless acted upon by an external force. • A body persists in a state of uniform motion or of rest unless acted upon by an external force. • A body keeps doing what its doing unless forced to change. • AKA: the law of inertia.

37. Newton’s Second Law of Motion • Force equals mass times acceleration. • net F = ma (formula sheet) • AKA: F = ma

38. Newton’s Third Law of Motion • To every action there is an equal and opposite reaction. • AKA: Action – Reaction Law • Action reaction pairs: • If John hits Joe. • Joe hits John.

39. Force • A force is a push or a pull. • Force is measured in Newtons, N , (n). • Weight is a force due to the pull of Earth’s gravity. • Weight = mass x acceleration due to gravity • Acceleration due to Earth’s gravity = 9.8 m/s2

40. Weight • Weight is a force due to the pull of Earth’s gravity. • Weight = mass x acceleration due to gravity • Acceleration due to Earth’s gravity = 9.8 m/s2 • Weight is measured in Newton’s; N, (n)

41. Friction • A force that acts against motion. • Measured in Newtons, N, (n)

42. Convection • A form of heat transfer through liquids and gases (fluids). • Heat is transferred by currents in the fluids. • Heat moved by fluid motion.

43. Conduction • Heat transferred by vibrating neighboring molecules. • Heat transferred through solids. • Heat moves from hot to cold.

44. Radiation • Heat transferred by waves. • Heat from our Sun reaches us through waves.

45. Reflection • When a wave hits a barrier it bounces off at the same angle it hits the surface. • When you look in the mirror you see your reflection. • The law of reflection is the angle of the incoming ray equals the angle of the out going ray.

46. Refraction • When a light ray changes mediums it bends. The bending of alight ray is refraction. • When a wave changes mediums it refracts. • The change of direction of a ray of light, sound, heat, or the like in passing from one medium into another due to the change in the speed of the wave.

47. Diffraction • The change in a wave as it passes by an obstacle or through an opening. • The spreading out of a wave as it passes by a barrier.

48. Resonance • Also called sympathetic vibrations. • Something starts to vibrate or shake because something else is vibrating.

49. Period, T • The amount of time it takes to do something once. • The amount of time to make one wave. • Period, T , is measured in seconds, s.

50. Frequency, f • Frequency, f , is how many things happen in one second. • How many waves are made in 1 second. • Frequency , f , is measured in Hertz, Hz.