Chemistry XI Unit 2 Questions: 90 Time Limit: 90 minutes Passing Score: 60% Start Quiz Chemistry XI Unit 2 Question 1 of 90 The wavelength associated with moving electron is given by: λ = h/mv λ = hv λ = v/h λ = m/hv Bohr's model is most applicable to: hydrogen-like ions polyelectronic atoms all atoms equally no atoms The maximum number of electrons in d orbitals is: 6 10 14 18 Which set of quantum numbers is not possible? n=2, l=1, ml=0 n=1, l=0, ml=0 n=3, l=3, ml=-1 n=2, l=1, ml=-1 The energy of a photon is given by: E = hv E = λ/h E = m/v E = c/λ Heisenberg's Uncertainty Principle states: electron position can be known precisely electron velocity can be measured accurately both position and momentum cannot be known simultaneously electrons have definite orbits The atomic radius of an element is: distance from nucleus to outermost shell average distance of nucleus from electron actual size of nucleus distance between atoms Ionization energy generally increases across a period because: nuclear charge increases atomic size increases number of electrons increases electrons are more shielded The ground state electron configuration of Fe is: [Ar]3d⁶4s² [Ar]3d⁵4s² [Ar]3d⁷4s¹ [Ar]3d⁸4s⁰ According to Aufbau principle, electrons fill orbitals in order of: increasing energy decreasing energy random manner same energy levels only The orbital with highest penetration is: 2s 2p 3s 3d Hund's rule states that: electrons pair up first electrons first occupy separate orbitals with parallel spins orbitals fill randomly all electrons are paired The Pauli Exclusion Principle states: no two electrons have same mass no two electrons can have identical quantum numbers electrons must be in same orbital all electrons are identical Shielding effect means: electrons shield nucleus charge protons attract electrons electrons repel each other neutrons affect nuclear charge Across a period, electronegativity: decreases increases remains same varies randomly An orbital is best described as: pathway of electron energy level region of space with high probability of finding electron circular path around nucleus The quantum number that specifies energy level is: n l ml ms The angular momentum quantum number l can have values: 0 to n-1 0 to n 1 to n 0 only The spin quantum number ms can be: 0 only +1/2 and -1/2 any value +1 and -1 Which of the following is isoelectronic with Ar? K⁺ Ca²⁺ S²⁻ all of above The radius of d orbitals is generally: same as s orbitals smaller than p orbitals larger than s and p orbitals zero at nucleus The number of nodal planes in dxz orbital is: 1 2 3 Photoelectric effect demonstrates: wave nature of light particle nature of light both wave and particle nature neither wave nor particle The characteristic X-ray is produced when: inner shell electron is removed and outer electron falls down outer electron is removed and inner electron falls down electron is accelerated atom is heated The frequency of X-ray produced is related to: atomic number by Moseley's law atomic mass number of neutrons neutron-proton ratio Bohr's first postulate states: electrons orbit nucleus in circular paths at definite energies electrons can orbit at any energy nucleus orbits electron no electrons in atoms The energy of electron in nth orbit of hydrogen is proportional to: 1/n 1/n² -1/n² -1/n The transition from n=2 to n=1 releases energy called: Lyman series Balmer series Paschen series Brackett series An excited electron can lose energy by: emitting photon absorbing photon changing mass merging with nucleus The shape of s orbital is: spherical dumbbell-shaped cloverleaf complex The shape of p orbital is: spherical dumbbell-shaped cloverleaf linear Electron transitions to lower energy state is: exothermic endothermic isothermal neither The maximum number of electrons possible in N shell (n=4) is: 4 8 18 32 Effective nuclear charge increases across a period due to: increased shielding decreased shielding more neutrons change in atomic radius The first ionization energy of noble gases is: very high very low medium zero Electron affinity is usually: negative positive zero infinity The element with highest electronegativity is: Cl F O N Diagonal relationship is observed in: p block d block s block transition metals Metallic character increases: down a group across a period left to right in period up a group The atomic structure as proposed by Rutherford contained: nucleus with orbiting electrons electrons in nucleus continuous positive charge positive nucleus with electrons Thomson's model of atom proposed: plum pudding model nuclear model planetary model orbital model The Balmer series corresponds to transitions ending at: n=1 n=2 n=3 n=4 The Rydberg constant (R) value is approximately: 1.097 × 10⁷ m⁻¹ 1.097 × 10⁻⁷ m⁻¹ 1.097 × 10⁻¹ m⁻¹ 1.097 × 10¹ m⁻¹ The wavelength of electron depends on: mass and velocity mass only charge only color only According to wave mechanical model, electron path is: well-defined not well-defined circular elliptical Which orbital can have maximum three lobes/petals? s orbital p orbital d orbital f orbital FILLBLANK:The _____ Principle states no two electrons in atom have identical quantum numbers. Pauli Exclusion Hund's rule Aufbau principle Heisenberg's FILLBLANK:The orbital that is closest to nucleus among all orbitals is _____ orbital. 1s 2s 1p 2p FILLBLANK:Across a period, atomic radius _____. decreases increases stays constant varies randomly FILLBLANK:The atom proposed by _____ contains a nucleus with orbiting electrons. Rutherford Thomson Bohr Dalton FILLBLANK:The _____ quantum number specifies orientation of orbital. magnetic (ml) principal (n) azimuthal (l) spin (ms) FILLBLANK:The shape of d orbital is _____. cloverleaf spherical dumbbell octahedral FILLBLANK:The _____ of element increases down a group. atomic radius atomic mass ionization energy electronegativity FILLBLANK:The _____ shows ν = R(Z-σ)(1/n₁² - 1/n₂²). Moseley's Law Rydberg equation Planck's Law Bohr's Law FILLBLANK:The s orbital has _____ nodal plane. zero one two three FILLBLANK:The spin quantum number is denoted by _____ and has values ±1/2. ms ml l n FILLBLANK:The _____ of an atom is its tendency to attract electrons. electronegativity atomic radius ionization energy electron affinity FILLBLANK:The Lyman series corresponds to transitions ending at _____. n=1 n=2 n=3 n=4 FILLBLANK:The maximum electrons in a shell is given by _____. 2n² n² 4n n³ FILLBLANK:The _____ is the energy required to add electron to atom. electron affinity ionization energy excitation energy dissociation energy TRUE/FALSE: All elements have negative electron affinity. TRUE FALSE TRUE/FALSE: Bohr's model successfully predicts spectra of polyelectronic atoms. TRUE FALSE TRUE/FALSE: The spin quantum number can be +1/2 or -1/2. TRUE FALSE TRUE/FALSE: Effective nuclear charge increases across a period. TRUE FALSE TRUE/FALSE: s orbitals have angular momentum. TRUE FALSE TRUE/FALSE: Photoelectric effect requires light above threshold frequency. TRUE FALSE TRUE/FALSE: Hund's rule applies to all atoms. TRUE FALSE TRUE/FALSE: Atomic radius increases across a period. TRUE FALSE TRUE/FALSE: Metallic character increases down a group. TRUE FALSE TRUE/FALSE: The Balmer series is in ultraviolet region. TRUE FALSE TRUE/FALSE: Frequency of X-ray depends on atomic number. TRUE FALSE TRUE/FALSE: de Broglie wavelength increases with electron velocity. TRUE FALSE TRUE/FALSE: Shielding effect protects outer electrons from nuclear charge. TRUE FALSE TRUE/FALSE: Noble gases have very high ionization energies. TRUE FALSE TRUE/FALSE: Ionization energy is always negative. TRUE FALSE TRUE/FALSE: Electron affinity is always positive. TRUE FALSE TRUE/FALSE: Electronegativity decreases down a group. TRUE FALSE TRUE/FALSE: Fluorine has higher electronegativity than oxygen. TRUE FALSE TRUE/FALSE: The maximum number of d electrons is 10. TRUE FALSE TRUE/FALSE: Pauli Exclusion Principle allows 4 electrons per orbital. TRUE FALSE TRUE/FALSE: Thomson discovered the nucleus. TRUE FALSE TRUE/FALSE: Ground state electron configuration uses lowest energy orbitals. TRUE FALSE TRUE/FALSE: All transition metals have (n-1)d electrons. TRUE FALSE TRUE/FALSE: An orbital can contain maximum 2 electrons. TRUE FALSE TRUE/FALSE: The angular momentum quantum number can be zero. TRUE FALSE TRUE/FALSE: Spectral line represents energy difference between levels. TRUE FALSE TRUE/FALSE: The Rydberg equation applies to all atoms. TRUE FALSE TRUE/FALSE: Uncertainty principle makes electron paths unpredictable. TRUE FALSE TRUE/FALSE: Wave-particle duality applies to electrons. TRUE FALSE TRUE/FALSE: The orbital angular momentum depends on l and ml. TRUE FALSE Previous Next Submit Quiz Want to save your progress? Create an account or log in to track your quiz scores! Register/Login