Final Review

==Smallest unit of matter:== Atom

==Element-== Pure substance, one elemental symbol, an elements particle is an atom, example: O2

1. definition: a pure substance that cannot be broken down into simpler stable substances and is made of one type of atom

==Extensive properties-== Depends on the size of the system or on the amount of matter that is present

1. examples mass, volume and amount of energy

==Intensive properties-== Does not depend on the size of the system or on the amount of matter that is present

1. examples melting point, boiling point, density, and the ability to conduct electricity

==Physical change-== a change in which one or more substances are converted into different substances; does not change the identity of the substance

1. shape change, change in state, making a solution that is not a chemical change, grinding, cutting, melting, and boiling

==States of matter-==

1. gas- particles are far apart, movement is constant random motion, they will always fill a container
2. liquid- not as close together as a solid, potential for movement, they wont fill a container
3. solid- tightly packed particles, vibrate in place, wont fill a container

==Chemical change-== A change in a substance that does not involve a change in the identity of the substance

1. color change, produce a gas, produce a precipitate(cloudy) and or energy change, produce a new substance

==Homogeneous mixture-== mixtures that are uniform in composition, one layer

==Heterogeneous mixture-== mixtures that are not uniform throughout, more than one layer

10. ==Mixture vs. compound-== mixures are a blend of two or more kinds of matter, each of which retains its own identity and properties and a compound is a substance that can be broken down into simple stable substances that are made from the atoms of two or more elements that are chemically bonded

11. ==Pure substance-== has a fixed composition and they are always homogeneous.

12. every sample of a given pure substance has exactly the same characteristics properties

13. every sample of a pure substance has exactly the same composition

14. ==Separation of mixtures==

15. distillation- separating liquids based on boiling point. Example, right answer to the foul water

16. decanting-separating a solid and a liquid by pouring off the liquid after the solid settles

17. filtering- separating a solid and a liquid; the liquid passes through the filter paper and the solid remains in the funnel. Example is charcoal and water

18. evaporation- a method to separate water from a dissolved solid

19. chromatography- passing a mixture through a medium where the components move at different rate. Example, pen colors flowing through a coffee filter

20. ==Properties of groups-== share same chemical and/or physical properties and share the same amount of valence electron

21. ==Periods-== they have the same amount of electron shells

22. ==Metal vs. nonmetal properties-== solids, conductive of heat and electric currents, shiny, malleable, ductile and nonmetals are gases/liquids, non conductive of heat and electric currents, brittle, non maliable and ductile

23. ==Noble gas properties-== unreactive, odorless, colorless, room temperature, valence electron is full making it unreactive

24. ==Nonmetals-== an element that is a poor conductor of heat and electricity ad on the right side of the periodic table

25. ==Nonmental properties-== non conductors, brittle, gas/liquid, non maliable and ductile

26. ==Variables-== change one varialbe (independent) which will affect another variable (dependent)

27. ==Quantitative vs qualitative-== qualitative are senses and quantitative are numerical

28. ==Observations-== collecting data, measuring, experimenting, communicating

29. ==Scientific method-== a series of steps followed to solve problems, including collecting data, formulating a hypothesis, testing the hypothesis and stating conclusions aka formulating theories that are supported by data; A logical approach to solving a problem and order of steps vary with problem

30. ==Theory== - hypothesis that has withstood repeated testing and it can be revised. An example is the atomic theory

31. ==Control-== stays the same

32. ==Metric units for volume-== m^3

33. ==Metric units temperatures-== celcius

34. ==Metric units prefixes-==

    1. Teva-10^12
    2. giga-10^9
    3. mega-10^6
    4. kilo-10^3
    5. hecto-10^2
    6. deca-10^1
    7. base-10^0
    8. deci-10^-1
    9. centi-10^-2

35. mili-10^-3

36. micro-10^-6

37. nano-10^-9

38. pico-10^-12

39. <<==Metric conversions== is it supposed to be problems<<

40. [[==Density*==[[

41. ==Density -== the ratio of the mass of a substance to the volume of the substance; often expressed as grams per cubic centimeter

42. ==Weight-== amount of gravitational pull on matter. It can change based on your planent

43. ==Metric unit mass-== kg

44. <<==Metric units vs English units- mass grams vs pounds==<<

45. ==Precision-== closeness or exactness among a set of dattevaa. only the last place value differs

46. ==Precision vs. accuracy-== accuracy is the closeness of a measurement to an accepted value and precision is the closeness among A SET OF DATA not the accepted value

47. <<==Significant figures-==<<

48. ==Significant figures multiplication/division-== the answer has the same number of sig figs as the least number of the problem

49. ==Significant figures==

50. [[==Volume*==[[

51. [[==Significant figures addition*==[[

52. [[==Scientific notation* if all the digits are signnificant then they have to be put in the notation==[[

53. [[==Scientific notation multiplication*==[[

54. ==Number of electrons, protons and neutrons in an atom-== one proton, neutron, and electron

55. <<==Symbol for an isotope of an element-==<<

56. ==Law of Multiple Proportions-== if 2 or more compounds are composed of the same 2 elements than the ratio of the masses of the second element combined with the a certain mass of the first elements is always a ratio of small whole numbers. The scientist was Dalton

57. ==Gold Foil Experiment-== Rutherford observed that 1 in 8000 were deflected back. This was not expected. The alpha particles hit something small and dense. This is called the nucleus. His model had protons in the nucleus and electrons outside

58. ==Dalton’s Atomic Theory-== all matter is composed of small particles called atoms, atoms of an element are identical in size, mass, and other properties, atoms cannot be subdivided,*,created, or destroyed, atoms of different elements combine in simple whole number ratios to form compounds, in chemical reactions, atoms are combined, separated, or rearranged

59. ==Law of Definite Proportions-== a single chemical compound contains the same elements in the exactly the same proportions by mass regardless of the size of the sample or the source of the compound, scientist is Proust

60. ==Law of Conservation of Mass-== mass is neither created nor destroyed during ordinary chemical reactions or physical changes. Scientist is Lavoisier

61. ==Thomson’s experiment-== he did the cathode ray tube. He observed that rays were deflected away from negatively charged objects aka electrons. His model is the chocolate chip cookie model

62. ==Mole-== Avogadro’s number which is 6.022 x 10^23

63. <<==Mole and mass- known the relationship/conversion factor==<<

64. ==Molar mass-== same numerical value as atomic mass. it is used as a conversion factor and it is four sig figs

65. [[==Converting moles to atoms*==[[

66. ==Molar mass units-== g/mole

67. [[==Converting moles to grams*==[[

68. ==Average atomic mass-== the weighted average of the atomic masses of the isotopes of an element. The unit is amu or u. First do mass x abundance= x. Do for all of your isotopes and then add the products. Round as you go (look at examples)

69. ==Atomic mass-== mass number = protons + neutrons

70. ==Balance nuclear equation-== look at notes and practice equations

71. ==Positron-== Greek letter B 0 at the top and +1 at the bottom

72. ==Alpha particle-== 4 at the top at 2 at the bottom with He

73. [[==Converting grams to moles*==[[

74. [[==Converting grams to atoms*==[[

75. ==Orbital notation-== Look at notes, In orbital notation, an unoccupied orbital is represented by a line, , with the orbital’s name written underneath the line. An orbital containing one electron is represented as ↑ . An orbital containing two electrons is represented as ↑↓ , showing the electrons paired and with opposite spin states

76. ==Orbital notation==

77. ==Quantum numbers-== numbers that specify the properties of atomic orbitals and the properties of electrons in the orbital

78. Principle Quantum Number-symbol is n, Indicates the main energy level around the nucleus, as n increases the electrons energy and average distance from the nucleus increases

79. Magnetic Quantum Number-indicates the orientation in space of the orbital, where on the x,y,z plane it is

80. Spin Quantum Number-spin state of the orbital, two electrons can exist in one orbital

81. ==Rules governing electron configuration==

82. Pauli Exclusion Principle-no two electrons can have the same 4 Quantum numbers

83. Aufbau Principle-electrons must occupy the lowest energy position

84. Hund’s Rule-each orbital has one electron before pairing can occur

85. <<==Emission of a photon-electron going from a exited to ground state, absorb energy to to to a exited energy level==<<

86. ==Line emission spectrum- in general or hydrogen==

87. [[==Calculating frequency from wavelength*==[[

88. [[==Calculating frequency from energy*==[[

89. }}==Photoelectric effect-== refers to the emmisions of electrons from when a metal shines on the metal. Light must contain the minimum amount of energy to emit electrons from the metal. Metals have a unique minium amount of energy needed to emit electrons}}

90. ==Ground state-== electrons drop to the original energy level

91. ==Angular momentum quantum number-== tells the shape of the orbital. s are spherical, p are penut/dumbell shape, d are double dumbel shape, and f are flower shape

==Highest occupied energy level in an atom-== valence electrons

==Electron configuration (2 questions)-== the arrangement of electrons in an atom

==Noble gas notation for electron configuration (2 questions)-== refers to an outer main energy level occupied, in most cases by eight electrons

==Inner shell electrons-==electrons that are not in the highest occupied energy level

<<==Frequency of the electromagnetic spectrum-== the number of waves that pass a given point in a specific time, usually one second (do we need to know the types of waves)<<

==Wavelength== -the distance between corresponding points

==Dual nature of electromagnetic radiation-== light possesses both particle properties and wave properties

<<==Emission of photons==<<

<<==Number of orbitals on an energy level-n and square it and it would give you the number of orbitals==<<

==Orientation of orbitals- Magnetic Quantum numbers, where on the x,y,z axis, symbol is m==

==Spin quantum number- spin state of the orbital, two electrons can exist in one orbital==

==Mendeleev’s periodic table-== Mendeleev placed the following information on cards: name of element, atomic mass, and properties. He noticed that when elements were arranged in order of increasing atomic mass, similarities in their chemical properties occurred at regular intervals. He arranged the cards according to trends (patterns) in their properties (because it didn’t always fit based on atomic mass). Mendeleev left blank spaces in his periodic table for elements that were yet to be discovered. In addition, he predicted properties for those elements

==Groups-== colums in a periodic table

==Periodic law.-== The physical and chemical properties of the elements are periodic functions of their atomic number

<<==Electron configuration and groups- the electron configuration is the same but the number for the energy level differs==<<

==Outermost shell electrons-== the electron containing main energy level with the highest principal quantum number

==Group properties==

1. Alkali Metals properties-stored in oil, most reactive group, soft, low melting point, s block, react violently with water, highly reactive metals
2. Alkali Earth Metals properties- not as reactive as group 1, higher melting point than group 1, harder than group 1,
3. Transition Metals- metals that are solid, shiny, hard, and good conductors of electricity, they are found as free elements and they are not as reactive as group 1 and 2, d block, valence electrons are not predictable, makes color
4. Halogens- reacts with metals to form salts, most reactive non metal,
5. Noble gases- group 18, unreactive because they have a complete valence shell,
6. Lanthanides- atomic number 58-71, metal and has the qualities of one, similar reactivity to group 2, fills 4f,
7. Actinides- atomic number is 90-103, all elements are radioactive, 1st four are naturally occurring

==Group names==

1. Alkali Metals group number-group 1
2. Alkali Earth Metals group number- group 2
3. Transition Metals group number-group 3-12
4. Halogens group number-group 17
5. Noble Gases group number-group 18
6. Lanthanides atomic numbers-atomic number 58-71
7. Actinides atomic number-atomic number 90-103

==Electron configurations of main group elements==

==Transition metals-== metals that are solid, shiny, hard, and conductors, they are found as free elements and they are not as reactive as group 1 and 2, d block, valence electrons are not predictable, makes color

==Alkali metals-==Group 1, stored in oil, most reactive group, soft, low melting point, s block

==Electronegativity-==a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound.

==Atomic radius trend-== it increases to the left in a period and down a group

==Electronegativity trend-== it increases to the right in a period and goes up a group

==Ionization energy trend-== it increases to the right in a period and goes up a group

100. ==Electron affinity trend-== it increases to the right in a period and goes up a group

101. ==Noble gas configurations-== an outer main energy level occupied, in most cases by eight electrons

102. ==Electron configurations  and period-== the period can be determined from the elctron configuration. Look at the number in front of s or p and that will tell you which period or energy level it is

103. <<==Metals vs. nonmetals==<<

104. ==Electron configurations and p-block==

105. ==Reason for period trends-== group 13 starts as ns^2np^1 and group 18 ends as ns^2 np^8

     1. Group(vertical column)
     • adding electrons to sublevels in higher energy levels.
     • when inner shell electrons go up then electron shielding goes up
     • if you have a smaller size atom, the distance between the valance electrons and the nucleus is small and therefore increased the force of attraction
     1. Period (horizontal row)
     • adding electrons to the same energy level gives you the same number of inner shell electrons and the electron shielding stays the same
     • increasing the number of protons increases the nuclear charge which increases the force of attraction

106. Negative electron affinity

107. <<==Sublevels and loss of Electrons for transition element==<<

108. ==Groups and attraction for electrons-== the more valence electrons there are, the less likely they are to attract electrons, also known as electronegativity

109. <<==Comparing ionization energy==<<

110. <<==Metalloids==<<

111. <<==Ion charge==<<

112. <<==Octet rule, loss or gain of electrons==<<

113. ==ionic bonding-== chemical bonding that results from the electrical attraction between cations and anions

114. ==Ionic compound properties-== brittle, high melting/boiling point, strong electrical attraction between ions, solid at room temperature, do not conduct as a solid, ions are in a fixed positon, dissolve in water, conducts in water and as a liquid

115. <<==Recognizing polyatomic ions==<<

116. <<==Potential energy and bonding==<<

117. ==Melting points, ionic vs. molecular-== ionic bonds have high melting and boiling points and molecular bonds have low melting and boiling points

118. ==Covalent bonding-== results from the sharing of electron pairs between two atoms. Usually non metals

119. <<==Bond length==<<

120. <<==Bond energy==<<

121. <<==Determining type of bonds==<<

122. <<==Determining type of bonds==<<

123. <<==Resonance structures==<<

124. <<==Ionic character and electronegativity==<<

125. <<==Potential energy and stability==<<

126. <<==Lewis Structures==<<

127. <<==Lewis Structures==<<

128. <<==Metallic Bonding==<<

129. <<==Shape of Molecules==<<

130. <<==Shape of Molecules==<<

131. <<==Polar Molecules==<<

132. <<==Boiling point, polarity, and IMF==<<

133. <<==Intermolecular Forces==<<