1. Substitute the word “average kinetic energy” for “___________” to make questions easier. Temperature

2. Sublimation is a phase change from a _____directly to a____ 2. Sublimation is a phase change from a _____directly to a____. Two examples: CO2 and I2 SOLID GAS

3. Solutions containing ions of elements ____ (group 3-11) are often colored. Example:_______ Transition CuSO4

4. Only two elements exist as liquids as STP. Hg(metal) & Br(non-metal)

5. Elements are arranged in the periodic table according to their __________ atomic number

6. The atomic mass of an element is the weighted average of the element naturally___________ occurring isotopes

7. The mass number of an atom is found by adding the ____________ number of protons + neutrons

8. One atomic mass unit (1 amu) is defined as exactly 1/12 the mass of Carbon-12

9. Atoms that become ions by losing electrons _______in size while those that gain e-______ decrease increase

10. The nuclear charge of an atom is the same as its number of _______ protons

11. The nucleons of an atom are those particles found in the__________ nucleus (protons & neutrons)

12. Molecular substances generally contain only covalent bonds, have low_____and are______ melting point soft.

13. Molecules with polar bonds may be non-polar because their shapes are__________ symmetrical

14. Carbon dioxide has 2-Double bonds and is nonpolar because it is _________(shape=linear) symmetrical

15. Memorize the 7 elements that are diatomic: H2 N2 O2 F2 Br2 I2 CI2

16. Memorize: 1 mole= ________ molecules= ______ grams= ______ liters (if it is a gas at STP) 6.02 x 1023 GFM 22.4

17. Water, NH3 and HF have unusually high boiling points due to strong intermolecular forces (H bonds)

melting points very hard 18. Network solids contain covalent bonds, have high ________and are _______. Example: diamonds melting points very hard

19. Elements in the same group have similar chemical properties because they have the same number of ____________ valence electrons

principle energy levels(shells) 20. Elements in the same period have the same number of ________________ principle energy levels(shells)

21. Metallic elements generally obtain a complete octet by losing electrons

22. The most metallic elements are located in the __________region of the periodic table lower left

“sea of mobile electrons” 23. Metals are good conductors of heat and electricity because of their _______________ “sea of mobile electrons”

24. Group 1 & 2 metals are so reactive they are found in nature as _____________and must be obtained by electrolysis found as compounds

25. Semi-metals are located stair bold line and exhibit _________ and __________properties metallic nonmetallic

high temperature low pressure 26. Gases behave most like ideal gases under conditions of _________and ________ high temperature low pressure

27. The two gases that behave most like ideal gases under any conditions are _____ and _____ H He

28. An __________is a substance that is capable of conducting electricity when dissolved in water electrolyte

29. Three examples of electrolytes are ____, ______and ______ NaNO3(aq) NaCl(aq) KCl(aq)

30. Salt contains ionic bonds and are easily identified because they contain a _______ and ________ metal and a nonmetal

31. Memorize and know the significance of LEO-GER and RED CAT –AN OX

32. Saturated hydrocarbons only contain elements of H & C and have all __________ single bonds

33. Chemical reactions are spontaneous when they are _________ and entropy increases exothermic

34. All reactions (especially redox reactions), there must be conservation of mass and ________ charge

35. Identify which diagram represent an element, compound, and a mixture z: mixture of two elements X: compound y: element

36. When one element changes to another, the process is known as transmutation

37. Isotopes of all elements with atomic numbers greater than 83 are _________ and decay over time. radioactive

38. Alpha and beta decay are examples of________ natural transmutation

conversion of mass energy 39. Fission and fusion both release large amounts of energy due to the ____________ to _________ conversion of mass energy

40. Intermolecular forces between hydrocarbons are generally _______ weak

41. Larger hydrocarbons have ___________ and higher ____________ and __________ stronger intermolecular forces (van der walls forces) higher melting and boiling point

42. Polar solutes generally dissolve in polar solvents 42. Polar solutes generally dissolve in polar solvents. The most common polar solvent is _____ H2O

43. As the _____________ of dissolved particles in the solution increases the boiling point increases and the melting point decreases. concentration

44. ____________affect the m. p. and b. p 44. ____________affect the m.p. and b.p. to a greater extent than molecular solutes, because they dissociate in H2O ionic solutes

45. Electrons must _______ energy to move to the excited state and __________ energy to move to the ground state. gain release

46. Rutherfold’s gold foil experiment revealed than an atom is made of mostly ________________ empty space

47. Equilibrium exist when the rate of forward and reverse reaction are equal

48. When a system is at equilibrium, the concentration of reactants and products are ____________ constant

49. Electronegativity is a measure of an atom’s attraction for ________________. electrons

50. Ionization energy is the energy required to ___________ an electron from an element. remove