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Transcript
Chapter #1-3 Review 1)! ! ! ! ! Define matter and energy. 2)! Summarize the four point in the Kinetic Molecular Theory 3)! ! What are the four states of matter? Draw a diagram and label the phase transitions between the states. ! Solid, liquid, gas, plasma 4)! ! ! ! ! a)! b)! Give one example of a qualitative property of matter. Give one example of a quantitative property of matter. a)! b)! Qualitative - “what type?” - blue, green, tall, short Quantitative - “How much?” - 6’1”, 170 lbs, 16 seconds Matter - anything that has a rest mass and occupies a volume Energy - anything that is not matter but can cause a change in matter ! two categories, kinetic and potential 5)! ! List the main points of each atomic theory. Dalton, Thomson, Rutherford and Bohr. ! ! ! ! ! Dalton - Atoms are hard featureless spheres. Each element has a unique kind of atom. Combinations of atoms make compounds ! ! Rutherford - Electrons are small negatively charged particles that orbit a small massive positively charged nucleus. Atoms are mostly empty space. ! ! Bohr - Electrons are located in shells. Electrons are negatively charged particles located in shells surrounding a small dense positively charged nucleus. 6)! Give the name, charge, location and mass for each subatomic particle. ! Proton!! +1! ! nucleus! ! 1.0 amu ! Neutron! 0! ! nucleus! ! 1.0 amu ! Electron! -1! ! shells! ! ! 1/1834 amu 7)! ! ! ! ! A previously unknown element has the following information: Atomic number = 117 Atomic mass = 290 Describe this element in terms of number of each subatomic particle and predict the most likely ionic charge. ! ! ! # protons = 117! ! ! # neutrons = 290-117 = 173!! # electrons = 117 Thomson - Atoms contain small negative particles called electrons. The background contains a postive charge to maintain neutrality. In the halogen column therefore ! Ionic Charge = -1 8)! Draw the Bohr model diagrams for the following species (**watch the charge**) ! a)! Mg! ! ! ! ! ! b)! N! ! c)! P3-! ! ! ! ! ! d)! Na1+! ! e)! S2- 9)! ! In terms of electrons, what is the primary difference between ionic and covalently boned compounds? ! ! ! ! Covalent - electrons are shared between the two nuclei Ionic - one or more electrons are transferred from the metal atom to the ! non-metal atom creating ions, the ions are then electrostaticallt attracted ! to each other. 10)! Explain why elements want to form simple ions. What is the goal? ! All elements attempt to get a noble gas configuration of electrons. For very small elements they try to get 2 electrons like helium, for all larger elements the goal is 8 electrons in the valence shell. 11)! Name the following compounds ! ! ! ! ! ! ! a)! b)! c)! d)! e)! f)! g)! h) i)! j)! k)! ! ! ! ! 12) ICl3 ! ! N2O3! ! ! SO3! ! ! SeF2! ! ! Cd3N2! ! ! Fe3As2!! ! Ag2CO3 Ca3P2! ! ! Zn(NO3)2! ! PbCrO4! ! Pt(CH3COO)4! Iodine trichloride Dinitrogen trioxide Sulfur trioxide Selenium difluoride Cadmium (II) nitride Iron (III) arsenide Silver carbonate Calcium phosphide Zinc nitrate Lead (II) chromate Platinum (IV) acetate Give the formula for each compound (**watch endings**) a) b) c) d) e) f) g) h) carbon diarsenide tetrasufur dinitride nitrogen trichloride calcium fluoride technetium (IV) sulphide tin (IV) carbonate antimony (V) nitrate manganese (II) chlorite CAs2 S 4N 2 NCl3 CaF2 TcS2 Sn(CO3)2 Sb(NO3)5 Mn(ClO2)2 13) List four difference evidences for a chemical change. ! ! ! New colour! ! New odour! ! ! ! Change of phase (eg solid or gas formed) New texture 14)! Classify each reaction in terms of; ! a)! chemical versus physical! ! b)! ! i)! Frying an egg! chemical & endothermic ! ii)! Burning natural gas in a furnace! chemical & exothermic ! ! iii)! ! Lifting a text book from the floor to the table! ! ! ! ! ! physical & endothermic ! ! iv)! ! Two solutions are mixed and the resulting mixture begins to glow green ! ! ! ! ! chemical & exothermic ! v)! A candle burning! ! vi)! Recharging the battery on a cellphone! ! ! ! ! exothermic versus endothermic chemical & exothermic chemical & endothermic
