Fall 2024 Chemistry Midterm PDF

Fall 2024 Chemistry Midterm 1) The nucleus of an atom contains __________. a) protons b) electrons c) protons and neutrons d) protons and electrons e) protons, neutrons, and electrons 2) Potassium is a __________ and chlorine is a __________. a) nonmetal, metal b) metal,...

Fall 2024 Chemistry Midterm 1) The nucleus of an atom contains __________. a) protons b) electrons c) protons and neutrons d) protons and electrons e) protons, neutrons, and electrons 2) Potassium is a __________ and chlorine is a __________. a) nonmetal, metal b) metal, nonmetal c) metal, metalloid d) metalloid, nonmetal e) metal, metal 3) Predict the empirical formula of the ionic compound that forms from aluminum and sulfur. a) AlS b) Al3S2 c) Al2S3 d) AlS2 e) Al2S 4) The correct name for SrO is __________. a) strontium dioxide b) strontium oxide c) strontium monoxide d) strontium peroxide e) strontium hydroxide 5) The name of PCl3 is __________. a) trichloro potassium b) potassium chloride c) monophosphorous trichloride d) phosphorous (III) chloride e) phosphorous trichloride 6) The formula of ammonium carbonate is __________. a) N2 (CO3 )3 b) (NH4 )2CO3 c) (NH3 )2 CO3 d) (NH3 )2CO4 e) NH4CO2 7) Chromium and chlorine form an ionic compound whose formula is CrCl3. The name of this compound is __________. a) chromic trichloride b) chromium chlorine c) chromium (III) trichloride d) monochromium trichloride e) chromium (III) chloride 8) Of the following, the smallest and lightest subatomic particle is the __________. a) alpha particle b) neutron c) nucleus d) electron e) proton 40 9) There are _________ electrons, _________ protons, and _________ neutrons in an atom of 18Ar. a) 40, 40, 18 b) 68, 40, 18 c) 54, 54, 78 d) 78, 78, 54 e) 18, 18, 22 10) Isotopes are atoms that have the same number of _______ but differing number of _______. a) neutrons, electrons b) protons, electrons c) electrons, protons d) protons, neutrons e) neutrons, protons 11) The element Si has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table to the right. The average atomic mass of the element is __________ amu. a) 25.82 b) 220.4 c) 2810.88 d) 28.1 e) 220.42 12) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? a) Si, P b) O, S c) H, He d) K, Ca e) C, N 13) Which of the following compounds would you expect to be ionic? a) CaO b) SF6 c) NH 3 d) H 2 O2 e) H 2 O 14) Which pair of elements is most apt to form a molecular compound with each other? a) barium, bromine b) aluminum, oxygen c) potassium, lithium d) sulfur, fluorine e) magnesium, iodine 15) Which one of the following compounds is chromium(III) oxide? a) Cr2 O 4 b) Cr2O3 c) Cr3O d) Cr3O2 e) CrO3 16) The wavelength of light that has a frequency of 1.20  1013 s 1 is __________ m. a) 2.5 b) 25.0 c) 12.0 d) 0.0400 e) 2.50  105 17) What is the frequency (s1 ) of electromagnetic radiation that has a wavelength of 0.53 m? a) 1.3  1033 b) 5.7  108 c) 1.3  10 33 d) 1.6  108 e) 1.8  109 18) Of the following, __________ radiation has the shortest wavelength. a) infrared b) X-ray c) ultraviolet d) microwave e) radio 19) The wavelength of a photon that has an energy of 5.25  10 19 J is __________ m. a) 3.79  107 b) 3.79  107 c) 4.21 10 24 d) 2.38  1023 e) 2.64  106 20) The energy of a photon that has a wavelength of 12.3 nm is __________ J. a) 1.62  1017 b) 1.511017 c) 2.72  1050 d) 1.99  1025 e) 4.42  1023 21) An electron cannot have the quantum numbers n = ______, l = ______, ml = ______. a) 3, 2, 1 b) 2, 0, 0 c) 1, 1, 1 d) 3, 1, -1 e) 2, 1, -1 22) Which one of the following represents an acceptable set of quantum numbers for an electron in an atom? (arranged as n, l, ml, and ms) a) 3, 3, 3, -1/2 b) 2, 2, -1, -1/2 c) 5, 4, -5, 1/2 d) 3, 3, 3, 1/2 e) 1, 0, 0, 1/2 23) Which one of the following is the correct electron configuration for a ground-state nitrogen atom? A) B) C) D) E) None of the above is correct. 24) There are __________ orbitals in the third shell. a) 1 b) 25 c) 9 d) 16 e) 4 25) The lowest energy shell that contains f orbitals is the shell with n = __________. a) 5 b) 3 c) 1 d) 4 e) 2 26) How many quantum numbers are necessary to designate a particular electron in an atom? a) 5 b) 3 c) 1 d) 2 e) 4 27) There are __________ unpaired electrons in a ground state phosphorus atom. a) 4 b) 0 c) 3 d) 2 e) 1 28) The ground state electron configuration for Zn is __________. a) [Kr]3s2 3d10 b) [Kr]4s2 3d10 c) [Ar] 4s23d104p4 d) [Ar]4s1 3d10 e) [Ar]4s2 3d10 29) The largest principal quantum number in the ground state electron configuration of barium is ____. a) 6 b) 1 c) 5 d) 4 e) 2 30) Which set of three quantum numbers (n, l, ml) corresponds to a 3d orbital? a) 2, 3, 3 b) 3, 2, 2 c) 2, 1, 0 d) 3, 2, 3 e) 3, 3, 2 31) At maximum, an s-subshell can hold __________ electrons, a p-subshell can hold __________ electrons, and a d-subshell can hold __________ electrons. a) 2, 6, 10 b) 14, 10, 6 c) 2, 12, 21 d) 14, 8, 18 e) 2, 8, 18 32) Elements in the modern version of the periodic table are arranged in order of increasing _______. a) number of isotopes b) oxidation number c) atomic number d) average atomic mass e) atomic mass 33) In which set of elements would all members be expected to have very similar chemical properties? a) Ne, Na, Mg b) O, S, Se c) S, Se, Si d) Na, Mg, K e) N, O, F 34) Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger __________ in Ar. a) azimuthal quantum number b) nuclear charge c) Hund’s rule d) diamagnetism e) paramagnetism 35) Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar? a) Ar > P > Si > Mg > Na b) Mg > Na > P > Si > Ar c) Na > Mg > Si > P > Ar d) Si > P > Ar > Na > Mg e) Ar > Si > P > Na > Mg 36) The atomic radius of main-group elements generally increases down a group because __________. a) both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases b) effective nuclear charge increases down a group c) the principal quantum number of the valence orbitals increases d) effective nuclear charge zigzags down a group e) effective nuclear charge decreases down a group 37) Which one of the following atoms has the largest radius? a) Ne b) O c) Cl d) S e) F 38) Which one of the following has the smallest radius? a) Br b) Na c) P d) Fe e) Cl 39) Which of the following is an isoelectronic series? a) O2- ,F, Ne,Na  b) B5- ,Sr 4- ,As3- ,Te2- c) Si 2- ,P2- ,S2- ,Cl2- d) S, Cl, Ar, K e) F , Cl ,Br  ,I 40) Which of the following correctly lists the atoms in order of increasing size (smallest to largest)? a) F < Br < Ge < Rb < K b) F < K < Ge < Br < Rb c) F < Br < Ge < K < Rb d) F < K < Br < Ge < Rb e) F < Ge < Br < K < Rb 41) Of the choices below, which gives the order for first ionization energies? a) S > Si > Cl > Al > Ar b) Cl > S > Al > Ar > Si c) Cl > S > Al > Si > Ar d) Al > Si > S > Cl > Ar e) Ar > Cl > S > Si > Al 42) Of the following elements, which has the largest first ionization energy? a) Ge b) F c) Sb d) S e) As 43) Which of the following has the largest second ionization energy? a) P b) Si c) Li d) Al e) Mg 44) Which equation correctly represents the first ionization of aluminum? a) Al (g)  e Al(g) b) Al (g) Al(g)  e c) Al(g) Al + (g)  e- d) Al(g)  e  Al- (g) e) Al(g) Al- (g)  e  45) Which ion below has the largest radius? a) Na  b) Cl  c) F d) Br  e) K  46) Of the following elements, __________ has the greatest electronegativity. a) O b) Na c) N d) Be e) Li 47) The list that correctly indicates the order of metallic character is __________. a) Na > K > Rb b) B > N > C c) P > S > Se d) Si > P > S e) F > Cl > S 48) Based on the octet rule, bromine most likely forms a __________ ion. a) Br+ b) Br2- c) Br2+ d) Br- e) Br3- 49) Based on the octet rule, strontium most likely forms an __________ ion. a) Sr+ b) Sr2- c) Sr2+ d) Sr- e) Sr3- 50) How many unpaired electrons are there in the Lewis structure of a nitrogen atom? a) 0 b) 3 c) 2 d) 1 e) This cannot be predicted 51) The alkaline earth metals, halogens, and alkali metals have __________ valence electrons, respectively. a) 2, 7, and 4 b) 7, 4, and 6 c) 7, 1, and 2 d) 8, 2, and 3 e) 2, 7, and 1 52) Which of the following would have to lose one electron in order to achieve a noble gas electron configuration? O Sr Na Se Br a) Sr, O, Se b) O, Se c) Br d) Na e) Sr 53) Elements from opposite sides of the periodic table tend to form __________. a) covalent compounds that are gaseous at room temperature b) covalent compounds c) homonuclear diatomic compounds d) compounds that are gaseous at room temperature e) ionic compounds 54) The Lewis structure of H2O shows __________ nonbonding electron pair(s) on oxygen. a) 3 b) 2 c) 1 d) 0 e) This cannot be determined from the data given 55) Which of the following does not have eight valence electrons? a) Ca2+ b) Rb  c) Xe d) Br  e) All of the above have eight valence electrons. 56) In the Lewis symbol for a chlorine atom, there are __ paired and __ unpaired electrons. a) 7, 0 b) 6, 1 c) 1, 6 d) 2, 4 e) 4, 2 57) The most common sulfur ion has a charge of __________. a) 2- b) 1- c) 4+ d) 6+ e) Sulfur does not form ions. 58) How many protons, neutrons, and electrons are in the following atom: 34S2-? a) 16 protons, 18 neutrons, 18 electrons b) 16 protons, 16 neutrons, 16 electrons c) 16 protons, 16 neutrons, 18 electrons d) 18 protons, 16 neutrons, 18 electrons e) 18 protons, 16 neutrons, 16 electrons 59) How many hydrogen atoms must bond to silicon to give it an octet of valence electrons? a) 1 b) 2 c) 3 d) 4 e) 5 60) What is the correct ground-state electron configuration for Nickel? a) [Ne] 4s2 3d8 b) [Ar] 3s2 3d8 c) [Ar] 4s2 3d8 d) [Ar] 4s2 4d8 e) [Kr] 4s2 3d8