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Name: ____________________________ Chemistry 2016 Mid-term Study Guide Chemistry Skills Convert each of the following: 345 mL = ____________ L 2.315 g = ____________ mg 421 cm = ____________ mm 0.0567 km = ____________ m 1.0 x 10-2 L = ______________ L What is the metric base unit for: Mass? ________________ Wet Volume? _______________ Distance? _______________ The metric prefixes from largest to smallest are kilo-, hecta-, deca-, deci-, centi- and milli-. A __________________ has definite volume and definite shape. A __________________ has definite volume but takes the shape of its container. A __________________ has neither definite volume nor definite shape. Label each of the following as a physical or chemical property. Shape physical or chemical Melting Point physical or chemical Reactivity with Acid physical or chemical Density physical or chemical Speed physical or chemical Boiling Point physical or chemical Odor physical or chemical Flammability physical or chemical In a ________________ change, the physical properties are adjusted (size, shape, density) but the chemical composition remains the same. In a ________________ change, the result is the formation of one or more new substances with different chemical properties. A change of state is not a _______________ change because the chemical identity of the substance has not been altered. Water that is frozen has not undergone a chemical change because it is still ___________________. Classify the following as a physical or chemical change. Burning wood physical or chemical Dissolving salt physical or chemical Cutting paper physical or chemical Freezing water physical or chemical Melting iron physical or chemical An _____________________ is a pure substance that cannot be broken down by ordinary chemical means into simpler substances. A ______________________ is a substance consisting of two or more different elements in definite proportions joined by chemical bonds. The elements cannot be separated by physical means. A ______________________ is a substance consisting of two or more elements or compounds that can be separated by physical means. A _______________________ mixture is a combination of two or more substances that has uniform composition and properties throughout. A _______________________ mixture is a combination of two or more substances that does not have uniform composition and properties throughout. Classify the following as element, compound, homogeneous mixture or heterogeneous mixture. Copper ____________________________ Milk ______________________________ Nitrogen ___________________________ Water _____________________________ Orange juice with pulp ____________________________________ The density of a liquid equals the mass/volume or D = m/V. Solving for mass, m = __________and solving for volume, V = __________________. Density remains the __________ when the quantity of a substance changes and its units are _____________. Precision describes how consistent a set of _________________________ are to each other. Accuracy describes how close a set of measurements are to the accepted __________. Atomic Structure What subatomic particles have significant mass? _________________ and ______________. Where is the majority of the mass of an atom? ______________________. Atoms of the same element with different mass numbers are known as ________________. The atomic number equals the number of _________________ in the nucleus. In neutral atoms, the number of protons equals the number of ______________________. The atomic mass equals the number of ________________ and __________________. The charge on an element is equal to the number of _______________ minus the number of _____________________. The average atomic mass is the sum of all of the masses of the different _______________of the element multiplied by their percent abundance. This causes atomic masses reported in the periodic table not to be _________ numbers. Ions are atoms that have an unequal number of __________________ and _________________. Ions that are negative have _________ electrons than protons and are called ________________. Ions that are positive have _________ protons than electrons and are called ________________. In the following, 41Ca2+ What is the charge? __________ What is the mass number? __________ How many protons? __________ How many neutrons? __________ How many electrons? __________ In the following, 33P3What is the charge? __________ What is the mass number? __________ How many protons? __________ How many neutrons? __________ How many electrons? __________ Electron Configuration The s orbitals are shaped like a _________________. The p orbitals are shaped like a _____________________. Most of the d orbitals are shaped like a double ______________________. When n =1, the total number of electrons can be ______. When n =2, the total number of electrons can be ______. When n= 3, the total number of electrons can be ______. What does “n” stand for? ________________ _________________. What is the complete electron configuration for: Ca ___________________________________________________ P…___________________________________________________ Cu ___________________________________________________ What is the abbreviated (noble gas) configuration for: Ga ___________________________________________ Na ___________________________________________ Pb ___________________________________________ How many orbitals are available for each of the following: s? __________ p? __________ d? __________ f? ___________ Each individual orbital can hold _____ electrons. How many electrons can each of the following sublevels hold: s? __________ p? __________ d? __________ f? ___________ Each arrow in an orbital diagram represents an __________________. The direction of the arrow indicates the _________________. When drawing orbital diagrams, electrons fill orbitals with the ______________ energy first. For example, 2s is filled before 2p. When drawing orbital diagrams, electrons fill subshells with multiple orbitals with _____ electron in each orbital spinning in the ________ direction before adding a second _____________ to the orbital. When drawing orbital diagrams, no two electrons in the same orbital can have the same __________. Please draw orbital diagrams for the following: Cr Si Periodic Table What is a vertical column in the Periodic Table called? ________________ What is a horizontal row in the Periodic Table called? _________________ The metals are to the _________ of the staircase on the Periodic Table. What are four properties of all metals? ____________________________ ____________________________ ____________________________ ____________________________ What is the charge of all metal ions (positive or negative)? ___________________ The nonmetals are to the ___________ of the staircase on the Periodic Table. Several nonmetals are gases. What are four properties of nonmetals? ____________________________ ____________________________ ____________________________ ____________________________ What is the charge of all nonmetal ions (positive or negative)? ___________________ How many valence electrons do elements in the following groups have? Group 1? _______ Group 2? _______ Group 13? _______ Group 14? _______ Group 15? _______ Group 16? _______ Group 17? _______ Group 18? _______ What is the charge (number and sign) for ions from each of the following? Group 1? ________ Group 2? ________ Group 13 metals? ________ Group 15 nonmetals? ________ Group 16 nonmetals? ________ Group 17 nonmetals? ________ What is the name for each of the following sections of the Periodic Table? Group 1? ________________________________ Group 2? ________________________________ Group 17? _______________________________ Group 18? _______________________________ The noble gases are known to be stable or _______________________. The metalloids are found along the staircase of the Periodic Table and are also called _______________________________ or semimetals. What is the oxidation number (charge) of sodium in NaCl? _________ Periodic Trends The number of energy levels of a neutral atom is the same as its ___________________. Moving down a group on the Periodic Table, the atomic radius (size) ____________________. This is because higher energy orbitals are being added which are _____________ from the nucleus. Moving across a period on the Periodic Table, the atomic radius (size) ___________________. This is because the increase in number of protons creates a stronger pull on the _______________ electrons. As atomic radius increases, does the force to remove an electron become higher or lower? __________________. This happens because electrons that are _______________ from the nucleus are _________________ to remove. What is the term for the force to remove an electron? _________________________ ________________. As atomic radius increases, does the ability of an atom to pull electrons towards itself become higher or lower? _______________. This happens because electrons that are ____________ from the nucleus are _______________ to remove. What is the term for an atom’s ability to attract electrons towards itself? __________________________________. Which of the following has a higher electronegativity? Rb or Na? _____________ N or P? _______________ S or Cl? _______________ F or K? _______________ Which of the following has a higher ionization energy? Mg or Ba? _____________ O or S? _______________ Br or Cl? ______________ Fr or F? _______________ In the reactivity lab, Ca was more reactive than Mg because as you go down a group in the Periodic Table it becomes ___________ for a metal to ________ its valence electrons. Bonding Describe the electron sharing (equal, unequal or none) for the following: Ionic Bonds ____________________ Polar Covalent Bonds _________________ Nonpolar Covalent Bonds __________________ To determine the amount of electron sharing, you determine the electronegativity ___________________ between the two atoms. If the two atoms have the same _________________________, the difference will be _______ and they will have ____________ sharing of electrons and it will be a __________________ covalent bond.