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Chapter 4 and 5 Test Review 1) Define the following: a. Proton- Positive charge particle in nucleus b. Neutron-neutral charge particle in nucleus c. Electron- negative charge particle outside nucleus d. Atom- the smallest particle of an element that retains the properties of that element e. Ion- Atom with a different number of protons and electrons f. Isotope- two atoms of same element that have differing number of neutrons. g. Nucleus- Center of atom. Contains the protons and neutrons. h. mass number- sum of the protons and neutrons in an atom. i. atomic number- indicates the number of protons in an atom. j. atomic mass- weighted average of all of the different isotopes of an element. k. atomic orbital- region of high probability of finding an electron l. aufbau principle- tendency of electrons to enter orbitals of lowest energy first m. Hund’s Rule- every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin. n. electron configuration- the arrangement of electrons in an atom. o. ground state electron- electron in its lowest energy state p. Pauli exclusion principle- no two electrons can occupy the same place in an atom (cannot have the same 4 quantum numbers.) q. Heisenberg uncertainty principle- you cannot know the location and velocity of an electron at same time. r. atomic emission spectrumfrequencies of light emitted by an element. s. Frequency- number of wave cycles per second (s-1) t. Wavelength- distance from equivalent points on two different waves (m) u. Photon- discrete bundled of electromagnetic energy 2) Know the theories or models presented by the following scientists. a. Democritus- coined the term atomos b. Dalton- 4 theories of atom i. Atoms cannot be broken down ii. Different elements have different masses iii. Elements combine to form compounds iv. Chemical reaction rearranges atoms. Cannot form atoms with partial elements. c. Thompson- found electron. Chocolate chip cookie model of atom. d. Rutherford- found nucleus e. Bohr- Planetary model of the atom. Rings are fixed energy levels. f. (Know what the cloud model states) 3) Using the periodic table fill in the spaces below. Atomic # Symbol Mass # Charge # Protons # Neutrons # Electrons 7 +1 3 4 2 N 14 -3 7 7 10 Co 59 0 37 32 27 I 127 -1 53 74 54 Au 118 . +3 79 118 76 3 7 7 14 27 53 79 Li 59 127 118 4) Explain what happens when an atom absorbs energy. Explain in terms of what the electrons do. - Electrons go from being in their ground state to being in their excited state. Immediately they fall back down to their ground state and emit the energy they absorbed. 5) What is the speed of light? How does it compare with the speed of other electromagnetic waves? - 3.00x108 m/s…all electromagnetic waves have the exact same speed. 6) What determines the color of light? How do the colors of light change with frequency and wavelength? - Color of light is determined by either the frequency or the wavelength. As frequency of wave goes up you move from red to violet. As wavelength goes up you move from violet to red. 7) Describe what is meant by atomic emission spectrum. Draw a picture if necessary. Energy given off by an atom as it releases absorbed energy. 8) What is the frequency of ultraviolet light with wavelength 2.94 - 10 m? (c = 3.00 10 m/s) F= c ÷ λ= 3.00x108 ÷2.94 x10-8 = 1.02 x1016 Hz 9) What is the wavelength of gamma ray electromagnetic radiation with a frequency of 2.73 Hz? (c = 3.00 10 m/s) 10 - λ= c ÷ F = 3.00x108 ÷ 2.74 x1020 = 1.09 x10-12 m 10) Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass number of 16.0 is 35.0% abundant; the isotope with a mass number of 21.5 is 65.0% abundant. What is the average atomic mass for element Z? (16*.35) + (21.5*.65) = 19.6 amu 11) Write the full electron configuration for: a. Potassium (K) - 1s2 2s2 2p6 3s2 3p6 4s2 b. Cadmium (Cd) - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 c. Phosphorous (P) - 1s2 2s2 2p6 3s2 3p3 d. Zirconium (Zr) - 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d2 12) Write the abbreviated electron configuration for: a. Cesium (Cs) - [Xe] 6s1 b. Hafnium (Hf) - [Xe] 6s2 4f14 5d2 c. Radium (Ra) - [Rn] 7s2 d. Niobium (Nb) - [Kr] 5s2 4d3 13) Determine the identity of the element using the electron configuration: a. 1s2 2s2 2p6 3s2 3p6 4s2 3d7 - Nickel b. [Kr] 5s2 4d10 5p3 - Antimony c. [Ne] 3s2 - Magnesium d. [Xe] 6s2 4f14 5d7 - Iridium 14) Determine the 4 quantum numbers for the outermost electrons for: a. Cesium (Cs) N=5 l=0 ml=0 ms=+1/2 b. Hafnium (Hf) N=5 l=1 ml=0 ms=+1/2 Radium (Ra) N=7 l=0 ml=0 ms=(-)1/2 Niobium (Nb) N=4 l=1 ml=1 ms=+1/2 15) What is meant by the term atomic orbital? a. What shape is an s orbital? -Spherical b. What shape is a p orbital? - Pear or dumbbell c. How many s orbitals are there? -1 d. How many p orbitals are there? -3 e. How many d orbitals are there? -5 f. How many f orbitals are there? -10