Chemistry PP Questions PDF

Chemistry PowerPoint Notes​ 1. What makes up everything in the universe? Matter makes up everything in the universe *Note made by me 2. Name 2 properties of all matter. Matter - Anything that occupies sp...

Chemistry PowerPoint Notes​ 1. What makes up everything in the universe? Matter makes up everything in the universe *Note made by me 2. Name 2 properties of all matter. Matter - Anything that occupies space or has mass. The 2 properties of all matter is mass and weight 3. Define mass. Quantity of matter an object has. 4. How does weight differ from mass? Weight is the pull of gravity on an object and mass is the amount of matter an object has. 5. What are elements? Elements are pure substances that can't be broken down chemically into smaller matter. 6. Name the 4 elements that make up most of a living thing. The 4 elements that make up most of a living things are oxygen, carbon, hydrogen, and nitrogen. 7. What is used to represent an element? An element is represented by an unique chemical symbol, that consists of 1-2 letters and the first letter is always capitalized. 8. Name the smallest part of an element. *Note by me The smallest part of an element is an atom. Properties of atoms - Determine the structure and properties of the matter they 9. What are the 2 main regions of an atom? compose. The 2 main regions of an atom are the nucleus and the electron cloud. 10. Where is the nucleus of an atom found and what does it contain? The nucleus of an atom is found at the center and it contains protons(positive charge) and neutrons(no charge). 11. What is the charge on a proton? A neutron? Protons have a positive charge and a neutron has a neutral charge. 12. All atoms of the same element have the ________ same number of protons. 13. The number of protons in an atom determines the *Note by me _________________________. Atomic Number Atomic mass is a decimal because it finds the average of all isotopes, 14. What is the charge on an electron? since there are different isotopes of Electrons have a negative charge. atoms. 15. If you know the number of protons in an atom, how can you determine the number of electrons? The number of protons and electrons are the same so you can determine the amount of electrons by only knowing the amount of protons. 16. Do all the atoms of the same element have the same number of neutrons? They could have the same amount of neutrons, but don't have to, but if they don't have the same amount of neutrons as their element is supposed to it will be an isotope. 17. Atoms of the same element with different numbers of neutrons are called ___________. isotope. 18. The mass of an atom is centered in the nucleus. ___________. 19. The number of protons PLUS neutrons in an atom determines its ___________________. atomic mass. 20. What atomic particle has a negative charge? An electron has a negative charge. 21. Why isn’t the mass of an electron used to determine the atomic mass of an element? Electrons aren't used to determine atomic mass because they have no mass. 22. Where are electrons found? Electrons are found outside the nucleus. 23. Which electrons in an atom have the most energy? Electrons in the outer energy levels have more energy than in the inner levels. 24. How many energy levels are there & name them? There are seven energy levels. They are K(closest to nucleus), L, M, N, O, P, and Q. 25. How many electrons will each energy level hold? K can hold 2 electrons and L-Q can only hold 8 electrons. 26. Elements are arranged on a __________________ Periodic Table by their atomic _____________. Number 27. What are Periods & what do they tell you about elements? The periods are horizontal rows on the periodic table and tell us the number of energy levels. 28.What are Families & what do they tell you about elements? The families & are the vertical groups and tell us the outermost number of electrons. 29. Two or more elements combined together make a _____________. compound 30. Chemical ______________ formula represent compounds. 31. _____________ Molecules are the smallest part of a compound. 32. ______________ Subscripts in chemical formulas tell the number of atoms of each element. 33. _____________ Coefficients in a formula tell the number of molecules. 34. Compounds have ____________ different properties than its elements. 35. The outermost _______________ number of electrons in elements determine if they will combine. 36. Elements with ___________ filled outer energy levels are stable & won’t react. 37. Why do elements tend to react with other elements? Elements tend to react with other elements to become more stable.(Chemical reactions) 38. Chemical _____________ equations represent chemical reactions. 39. ______________ products appear on the right of the equation, while ___________ reactants are on the left. 40. Chemical bonds store ____________. energy 41. How do covalent bonds form? Covalent bonds form when two atoms share one or more pairs of electrons. 42. How do ions form? Ions are formed when atoms lose or gain electrons. When atoms gain electrons they are negative ions but when they lose them they are positive ions. 43. Positive ions _________ lose electrons, while negative ions ___________ gain electrons. 44. Define energy. The ability to do work or cause change. 43. Give some examples of different forms of energy. Chemical, thermal, electrical, mechanical, and sound energy. 44. Atoms are in constant ________________, motion which determines the atom’s ____________. state 45. List the 3 main states of matter. Solid, Liquid, and gas  46. _______________ Thermal energy must be added or removed to change the state of matter. 47. In reactions the amount of product must ____________ be the same to the amount of reactants. *note by me 48. Most of an organism’s energy comes from _____________ sugar in foods. Reduction reaction - reactant gains 49. _______________ chemical reactions release energy. electrons becoming more 50. Give an example of an exergonic reaction in cells. Cellular respiration negative. 51. _________________ Endergonic reactions store energy. 52. Give an example of an endergonic reaction in cells. *Note by me Photosynthesis is an example of endergonic reactions. Oxidation reaction is when reactant *note by me loses electrons becoming more Catalysts in positive 53. Most reactions in cells are _________________. endergonic organisms are biological 54. _________________ activation energy is the energy needed to start a reaction. catalysts 55. Catalysts _____________ reduce the amount of activation energy needed. 56. Catalysts in organisms are called ______________ enzymes and are usually ______________. made up of proteins 57. Enzymes act on ____________ substrates which join at the _______________ active site. *Note by me 58. Can enzymes be reused? substrates are reactants in enzyme catalyzed Enzymes are reusable. reactions. 59. Define a solution. A solution is a mixture in which 2 or more substances are uniformly distributed in another substance. 60. The _____________ solute is dissolved in the ____________ solvent in a solution. 61. _______________ Water is the universal solvent. 62. A solution becomes _____________ saturated when no more solute will dissolve. 63. ______________ Aqueous solutions have water as the solvent & are important to ______________. to living things 64. What is the dissociation of water? Breaking apart of the water molecule into two ions of opposite charge(due to strong attraction of oxygen atom of one molecule for Hydrogen atom of another water molecule). *Note by me 65. Write the equation for this. concentration is the H2O 🡪 H+ (hydrogen ion) + OH- (hydroxide ion) measurement of the H+ + H2O 🡪 H3O (hydronium ion) amount of solute 66. OH is the ______________ hydroxide ion, while H+ is the ______________ hydrogen ion. Note by me 67. Acids produce _____________ hydronium ions, while bases have an excess of one of the important ________ hydroxide ions. aspects of a living system is the degree 68. The pH _______ scale measures the concentration of H+ ions and goes of acidity or alkalinity from ____________. 0-14 69. From 0 to 7 are ___________, acids a pH of 7 is __________, neutral & above 7 to 14 are _________. basic Buffers 70. _____________ are used in the body to control pH and keep it near a pH of ______ 7 or neutral. *Note by me Buffers also neutralize small amounts of acids or bases in a solution.