Units 1, 2 study guide- atomic structure

Transcription

1 Name: Units 1, 2 study guide- atomic structure 1) Complete the required information for each subatomic particle (T1.3) symbol name charge location Mass (AMU) p + e - n 0 2) Define the following terms: Cation (T1.3) anion (T1.3) isotope (T1.3) ion (T1.3) Orbital (T2.2) orbit (T2.1) valence electron (T2.3) isoelectric (T2.3) Ionization energy (T2.4) electronegativity (T2.4) 3) Which 7 elements are classified as metalloids (T1.4): 4) complete the table groups Name, if there is one # valence Charge of ion, if ions (T1.4) electrons (T2.3) are made (T2.3) Metals: Nonmetals: Nonmetals: Metals: 5) Give properties for each of the following groups of elements (T1.4) 1. Noble gases- 2. Alkaline earth metal- 3. Halogens- 4. Alkali metals- 5. Transition metals- 6) Which halogens are gases at room temperature, which is a liquid and which is a solid? (T1.4)G: L: S: 7) Which 3 of the above 5 groups of elements are so chemically active that they occur only as compounds in nature? (T1.4) 8) Give Noble gas core electron configurations for ions of the following elements, ion charges and nuclear charges for each (T2.3) Oxygen chlorine bromine magnesium sodium sulfur selenium nitrogen lithium calcium Identify all that are isoelectronic (there may be multiple groups of ions) (T2.3) 9) How much energy in kj (E) is required for the reaction: K + E K + + e -

2 9) An atom with 15 neutrons has two electrons in the first principal energy level, eight electrons in the second principal energy level and five electrons in the third principal energy level. From these data, supply the following values (T2.3, PS2.3) a) the mass number b) the atomic number c) standard isotopic notation d) complete electron configuration e) orbital diagram f) total number of electrons in p-orbitals g) number of vacant orbitals in the third PEL h) number of unpaired electrons i) total number of occupied orbitals k) total number of valence electrons l) nuclear charge 10) An ion with a charge of 1 and 18 neutrons has two electrons in the first principal energy level, eight electrons in the second principal energy level and eight electrons in the third principal energy level. From these data, supply the following values a) the mass number. b) number of protons c) standard isotopic notation d) complete electron configuration e) the total number of electrons in s-orbitals f) the total number of electrons in p-orbitals g) the noble gas with which this ion is isoelectric h) total number of valence electrons i) nuclear charge j) number of PELs completely filled 11) Each of the following represents either an atom or an ion. For each, give the element symbol and a charge (if there is a charge) (T2.3, PS2.3) Atomic # Electronic Configuration symbol (with appropriate charge, if needed) a) 12 1s 2 2s 2 2p 6 b) 20 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 c) 8 1s 2 2s 2 2p 6 12) Write the complete electron configuration for an atom of selenium (T2.3) 13) Draw an orbital level diagram (boxes with arrows) for an atom if selenium. Be sure to label the sublevels (1s, 2s, etc) (T2.3) 14) Write the Noble gas core configuration for an atom of selenium (T2.3) a) How many sublevels are completely occupied in the second principal energy level? b) How many sublevels are completely occupied in the third principal energy level? b) How many unpaired electrons does an atom of selenium have in the ground state? c) How many valence electrons does an atom of selenium have in the ground state?

3 15) Write the chemical symbol, along with appropriate charge, for two cations and two anions that are isoelectric with an ion of selenium (T2.3) Anions: Cations: 16) Write the complete electron configuration for an atom of polonium (Po) (T2.3) 17) a) How many orbitals are allowed in each subshell? (T2.2) s p d f b) Which is the highest energy sublevel in the 4 th PEL? 18) State, briefly, the basic description of the atom according to the following atomic models (scientist) a) Plum Pudding Model (T1.5) b) Wave Mechanical Model (T2.2) c) Nuclear Model (T1.5) d) Dalton s Atomic Model (T1.5) e) Planetary Model (T2.1) scientist- choose form Bohr, Rutherford, Dalton, Thomson; no name for wave mech. model. distinguish between the terms orbit and orbital = 19) Place the above models in historical order: earliest most recent 20) The density of a substance is 1.20 g/ml. What mass of the substance is contained in 1.25 L? (convert L ml first; 1000 ml per 1 L) (1.50 x 10 3 g) (T1.1) 21) A g sample of a substance has a volume of L. Calculate the density in g/ml. (1.98 g/ml) (T1.1) 22) The density of a substance is 1.20 g/ml. What volume is required to have 55.4 g of this substance? (46.2 ml) (T1.1) 23) The chemical properties of an atom are most closely related to the number of its (Protons, neutrons, valence electrons, or isotopes) (T2.3) 24) Give symbols for the seven diatomic elements (T1.4) 25) Write an equation to represent the first ionization energy for an atom of potassium. Include E for the energy, and e - for an electron on the appropriate sides of the equation (T2.4) Metals tend to and form Nonmetals tend to and form (gain or lose electrons, anions or cations) (gain or lose electrons, anions or cations) 26) Write the isotopic notation (T1.3) for an ion of: chlorine w/ 18 n 0 potassium w/ 21 n 0 sulfur w/ 19 n 0

4 27) Complete table with increases or decreases. (T2.4) Property Period (Left to Right) Group (Top to Bottom) Atomic radius Electronegativity First ionization energy 28) Calculate the atomic mass of potassium if the abundance and atomic masses of the isotopes making up its naturally occurring samples are as given below. (T1.3) Isotope Relative Abundance Atomic mass of the isotope Potassium % amu Potassium % amu 29) Calculate the atomic mass of magnesium based on the information provided below. (T1.3) Isotope Relative Abundance Atomic mass of the isotope Magnesium % Magnesium % Magnesium % ) From the following electron configurations, identify (T2.3) 1) ground state oxygen 2) excited state carbon 3) excited state oxygen 4) excited state nitrogen 5) ground state carbon 6) ground state nitrogen A) 1s 1 2s 2 2p 3 B) 1s 2 2s 2 2p 2 C) 1s 2 2s 2 2p 3 D) 1s 2 2s 1 2p 5 E) 1s 2 2s 1 2p 4 F) 1s 2 2s 2 2p 4 31) Complete table with increases or decreases (T2.4) 32) In period 2 which element has the greatest metallic character? Property Metallic character of elements nonmetallic character of elements Period (Left to Right), excluding noble gases Group (Top to Bottom) 33) In period 2 which element has the greatest nonmetallic character? 34) In group 14 which element has the greatest metallic character? 35) In group 14 which element has the greatest nonmetallic character? 36) Which is the most active nonmetal? 37) Which is the most active metal? 38) Which is the most active element in group 1? 38) Which group 1 element is the most chemically reactive? a) 1s 2 2s 2 2p 4 b) 1s 2 2s 2 c) 1s 2 2s 2 2p 5 d) 1s 2 2s 1 e) 1s 2 2s 2 2p 6 38) Of the above electron configurations, which would form ions with a: +1 charge -2 charge +2 charge -1 charge would not form ions 39) Give the number of orbitals in each subshell: s p d f 40) Spectral patterns result when electrons in excited states move from to (higher or lower) energy level and energy is (released or absorbed). 41) Explain the following with principles of atomic structure. (T2.4) a) An atom of Na has a larger atomic radius than an atom of argon. b) An atom of Na has a smaller atomic radius than an atom of K. c) An atom of Na has a lower first ionization energy than an atom of Cl.

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