Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
chem exam
| Question | Answer |
|---|---|
| Concerning the ground state of an atom, the electron configuration must obey which of the following rule(s)? Audbau Principle Pauli exclusion Principle Hunds rule | All three rules must be followed |
| Use definitions of n and ℓ to identify which of the subshells below do not exist due to the constraints upon the angular momentum quantum number? | 2d |
| Which of the subshells below do not exist due to the constraints upon the angular momentum quantum number? | All of them do exist. |
| Use definitions to identify which of the sets below is not a valid set of quantum numbers, (n, ℓ, mℓ)? | 4, 3, 4 |
| Which one of the following is not a valid value for the magnetic quantum number of electrons in a 3d, 4d, and 5d subshell? | 3 |
| Which of the subshells below do not exist due to the constraints upon the angular momentum quantum number? | All do not exist except 4f. |
| Calculate the energy (J) change associated with an electronic transition in a Bohr hydrogen atom from n = 3 to n = 1. Is the energy absorbed or released? | -1.94 × 10-18; released |
| Which of the following orbital is degenerate with 5py in a many-electron atom? | 5px |
| Which one of the following orbitals can hold two electrons? | All of them can hold two electrons. |
| Use definitions of n, ℓ, ml, and ms to identify which of the following is not a valid set of four quantum numbers, (n, ℓ, mℓ, ms)? | 1, 2, 0, +1/2 |
| Which element has the ground-state electron configuration as [Kr]5s14d5? | Mo |
| Which of the following contains a portion of wrong orbital energy? | 1s < 2s < 2p < 3s < 3p < 3d < 4s< 4p.... |
| Which of the following has the ground-state electron configuration as [Ar]4s13d5? | Cr |
| Which of the following is a valid set of four quantum numbers? (n, l, ml, ms) | 2, 1, 0, +1/2 |
| The valence shell of the element X contains 2 electrons in a 5s subshell. Below that shell, element X has a partially filled 4d subshell. What type of element is X? | transition metal |
| An electron cannot have the quantum numbers n = ________, l = ________, ml = ________. | 3, 2, 3 |
| An electron cannot have the quantum numbers n = ________, l = ________, ml = ________. | 1, 1, 1 |
| Which of the following electron configurations represents an excited state of carbon atom? | 1s22s22p13s1 |
| Which of the following atom has the ground-state electron configuration of as [Ar]4s13d5? | Cr |
| In a px orbital, the subscript x denotes the ________. | axis along which the orbital is aligned |
| Use definitions of n and ℓ to identify which one of the following is not a valid value for the magnetic quantum number of an electron in a 6d subshell? | 3 |
| Which of the following correctly indicates the order of metallic character? | Si > P > S |
| Of the elements below, ________ is the most metallic. | Cs |
| The ________ have the most negative electron affinities. | halogens (Group VII A) |
| Which ion has the smallest ionic radius? | Li+ |
| An alkali metal forms a compound with chlorine with the formula ________. | MCl |
| Which ionization process requires the most energy? | P3+(g) → P4+(g) + e- |
| Element M reacts with chlorine to form a compound with the formula MCl2. Element M is more reactive than magnesium and has a smaller radius than barium. This element is ________. | Sr |
| What is the ground-state electron configuration of the ion Cu2+? | [Ar] 3d9 |
| Of the following oxides, ________ is the most acidic. | SO2 |
| Which periodic table group contains only nonmetals? | 8A |
| Which periodic table group contains only metals? | 2A |
| List the elements Na, Ca, Rb, Cl, He in order of decreasing first ionization energy. | He > Cl > Ca > Na > Rb |
| Of the choices below, which gives the order for first ionization energies? | Kr > Br > Se > Ge > Ga |
| which element has the most favorable (most negative) electron affinity? | O |
| Which of the following is an isoelectronic series? | O2-, F-, Ne, Na+ |
| Which element is solid at room temperature? | I2 |
| The only noble gas that does not have the ns2np6 valence electron configuration is ________. | helium |
| Of the following metals, ________ exhibits multiple oxidation states. | Ni |
| In which set of elements would all members be expected to have very similar chemical properties? | Br, I, At |
| Of the following, which gives the correct order for atomic radius? | Na > Mg > Si > P > Ar |
| Which of the following correctly represents the third ionization of aluminum? | Al2+ (g) → Al3+ (g) + e |
| Which contains both covalent bonds and ionic bonds? | NH4Cl |
| Which two ions have the same electron configuration in the ground state? Hint: Isoelectronic species. | Ba2+ and I- |
| What species has the electron configuration [Ar]3d2? | V3+ |
| NO2– is be expected to have | two identical bonds intermediate between a single and a double bond |
| How many nonbonding electron pair(s) on As in the Lewis structure of AsH3? | 1 |
| What is the formal charge on N in NO3- in the Lewis structure below? | +1 |
| How many electrons are in the valence shell of I in IF4-? (aka How many valence electrons are on the central atom I?) | 12 |
| Which of the following has the bonds correctly arranged in order of increasing polarity? Electronegativity: F (4.0), O (3.5), N (3.0), Be (1.57), Mg (1.31) | O—F < N—F < Be—F < Mg—F |
| Which of the following does not have eight valence electrons? | Ca+ |
| Of the bonds C-C, CC, and C≡C, the C-C bond is ________. | weakest/longest |
| Which covalent bond is most polar? Given the electronegativity as following: H (2.1), F (4.0), C (2.5), O (3.5), Cl (3.0), P (2.2), Li (1.0) H-F F-F C-O P-Cl Li-F | H-F |
| Which molecule has the weakest bonds? Hint: Relationship between bond length and bond energy. | CI4 |
| Of the molecules below, the bond in ________ is the most polar. Electronegativity F (4.0), Cl (3.0), Br (2.8), I (2.5), H (2.1). | HF |
| Which bond should have the highest bond enthalpy (aka bond energy)? | N≡N |
| What is the enthalpy change of reaction for the reaction between chlorine and ethane that produces chloroethane and hydrogen chloride gases? | -114 kJ |
| The Lewis structure of N2H2 shows ________. | each nitrogen has one nonbonding electron pair |
| What is the electron configuration for the Co2+ ion? | [Ar]3d7 |
| Which is the longest bond? | N—N |
| Which molecule contains a triple bond? | HCN |
| Of the following elements, which has the lowest electronegativity? Hint: Periodic Trend. | Ca |
| Which of the following contains an atom that does not obey the octet rule? | ClF3 (chloride trifluoride) |
| The type of compound that is most likely to contain a covalent bond is ________. | one that is composed of only nonmetals |
| ClF3 has "T-shaped" geometry. There is/are ________ non-bonding domain(s) in this molecule. | 2 |
| What is the orbital hybridization on C of HCN? What is its molecular geometry? Is it polar or nonpolar? | sp; linear; polar |
| Which is the false statement concerning SiH2F2? | The molecule is nonpolar. |
| Which of the following has molecular geometry as seesaw? | SF4 |
| The molecular geometry of the BrO3- ion is ________. | trigonal pyramidal |
| Which of the following is nonpolar? | BF3 |
| Which is the nonpolar molecule? | CS2 |
| A typical triple bond consists of ________ sigma bond(s) and ______ pi bond(s). | 1, 2 |
| How many valence electrons are there on CO32-? | 24 |
| how many bonds and bonds in the molecule below? | 8 bonds and 3 bonds |
| Which of the following has resonance structure? | All have the resonance structures. |
| What is the electron-domain geometry, molecular geometry, and bond angle, respectively, for an NH4+? | tetrahedral; tetrahedral; 109.5o |
| What is the orbital hybridization and molecular geometry for the most right oxygen that bonded to hydrogen? | sp3; bent |
| What is the bond angles and orbital hybridization for SF4? | 90o, 120o, 180o and sp3d |
| What is the orbital hybridization, bond angle, and molecular geometry for the middle carbon that bonded to two oxygens in the structural formula of acetic acid? | sp2, 120o, trigonal planar |
| Which of the folliwng is wrong concerning the o and pi bonds? | pi bond is stronger than o bond. |
| What are the bond orders respectively concerning H2, He2, and H2+? | 1,0,1/2 |
| What are respectively the electron domain geometry, bond angle, orbital hybridization on Xe, and molecular geometry of XeF2? | Trigonal bipyramidal, 180o, sp3d, linear |
| Which of the following molecules or ions has identical electron-domain and molecular geometries? | CO32- |
Created by:
user-2004554