Relier Pairs CHEM 1305 Third Study QuizVersion en ligne CHEM 1305 Third Study Quiz par Julian Y. Ramírez 1 2 atoms, 1 lone pair 2 5 atoms, 1 lone pairs 3 2 atoms, 2 lone pairs 4 2 atoms, 3 lone pairs 5 5 atoms, 0 lone pairs 6 3 atoms, 1 lone pair 7 3 atoms, 0 lone pairs 8 4 atoms, 0 lone pairs 9 3 atoms, 2 lone pairs 10 6 atoms, 0 lone pairs 11 2 atoms, 0 lone pairs 12 4 atoms, 1 lone pairs 13 4 atoms, 2 lone pairs trigonal planar, bent trigonal bipyramidal, trigonal bipyramidal tetrahedral, tetrahedral tetrahedral, trigonal pyramidal tetrahedral, bent trigonal bipyramidal, distorted tetrahedron (seesaw) octahedral, square pyramidal trigonal bipyramidal, T-shaped trigonal planar, trigonal planar octahedral, square planar trigonal bipyramidal, linear octahedral, octahedral linear, linear 1 trigonal bipyramidal, trigonal bipyramidal bond angles 2 linear, linear bond angles 3 octahedrals' bond angles 4 axial 5 trigonal bipyramidal, linear bond angles 6 trigonal planar hybridization 7 tetrahedral, trigonal pyramidal bond angles 8 trigonal bipyramidal, distorted tetrahedron (see-saw) bond angles 9 tetrahedral hybridization 10 equatorial 11 octahedral hybridization 12 tetrahedral, bent bond angles 13 trigonal bipyramidal hybridization 14 trigonal planar, trigonal planar bond angles 15 trigonal bipyramidal, T-shaped bond angles 16 tetrahedral, tetrahedral bond angles 17 linear hybridization 18 trigonal planar, bent bond angles sp3d2 sp2 X-axis same as trigonal bipyramidal, trigonal bipyramidal bond angles 120 same bond angles as octahedrals 180 (trigonal bipyramidal) sp 105 sp3d 107 Y-axis 90,120,180 sp3 180 (linear) 118 109 90,180 1 Possible ms values 2 Spin quantum number 3 proposed that visible light consists of electromagnetic waves 4 ΔE= 5 Principal quantum number 6 Visible light wavelength 7 Possible ml values 8 Infrared, Microwaves, Radio Waves 9 Magnetic quantum number 10 the emission and transmission of energy in the form of electromagnetic waves 11 Speed of a wave= 12 Speed of light (c) 13 KE= 14 S orbital looks like _ ______ 15 Possible n values 16 Energy (light) is emitted or absorbed in these units 17 EM waves with the most energy and smallest wavelength 18 the distance between identical points on successive waves. 19 the number of waves that pass through a particular point in 1 second (Hz = 1 cycle/s). 20 UV, X-Rays, Gamma Rays 21 EM waves with the least energy and biggest wavelength 22 Light's nature 23 vertical distance from the midline of a wave to the peak or trough 24 E= 25 Quantum numbers 26 RH (Rhydberg constant) = 27 Possible l values 28 Planck's constant 29 Angular momentum quantum number 30 (for electromagnetic waves) λ × ν = E final - E initial Radio Waves ms h*v 450-750 nm 0,1,2,3 (n-1 max) n (n, l, ml, ms) ml Have a longer wavelength than the visible spectrum c +1/2,-1/2 Electromagnetic radiation l h=6.63*10^-34 J*s wave and particle nature Have a shorter wavelength than the visible spectrum 3.00*10^8 m/s Quanta 1,2,3,4,5,6,7 hv - W Maxwell Frequency (ν) -l,....,0,....,l Gamma Rays 2.18*10^-18 J λ × ν Amplitude a sphere Wavelength (λ) 1 Paramagnetism means 2 Covalent bond 3 electrons with the same values of n and l form a 4 Ionic bond 5 Lattice energy 6 Group 15 7 p orbital looks like _ ______ 8 Effective nuclear charge= 9 Cations are 10 Group 18 11 having the same number of electrons, and hence the same ground-state electron configuration 12 Diamagnetism means 13 Valence electrons 14 no two electrons in an atom can have the same four quantum numbers. 15 “Fill up” electrons in lowest energy orbitals 16 d orbital looks like _ ______ 17 Group one 18 Group 17 19 how the electrons are distributed among the various atomic orbitals in an atom. 20 When we draw lines to fill with electrons each line is an _______, electrons with the same values of n, l, and ml form an _______. 21 Representative elements 22 Ionization energy 23 Anions are 24 Ionization energy, electron affinity and electronegativity increase 25 Atomic radius increases 26 Group two 27 Electron affinity 28 Group 16 29 The most stable arrangement of electrons in subshells is the one with the greatest number of parallel spins 30 electrons with the same value of n form a _____ first, second and third will differ, the minimum energy (kJ/mol) required to remove an electron from a gaseous atom in its ground state. chalcogens atomic number - number of core electrons Hund’s rule halogens lower left Pauli exclusion principle a peanut the electrostatic force that holds ions together in an ionic compound. no unpaired electrons bigger than the normal element upper right Isoelectronic pnictogens negative of the energy change that occurs when an electron is accepted by an atom in the gaseous state to form an anion. chemical bond in which two or more electrons are shared by two atoms. the energy required to completely separate one mole of a solid ionic compound into gaseous ions. the electrons that participate in chemical bonding one or more electrons are unpaired orbital noble gases Aufbau principle a clover smaller than the normal element alkaline earths alkaline metals subshell s and p groups Electron configuration shell 1 These elements always follow the octet rule when drawing Lewis structures 2 Bring this 4 digit passcode to Julian for extra credit 3 Medium, fairly strong bond 4 Longest, weakest bond 5 Resultant dipole moments 6 Polar covalent bond 7 Shortest, strongest bond 8 Ionic bond 9 Hybridization 10 Nonpolar covalent bond 11 Electronegativity more than 0.5, less than 2.0 difference in electronegativity single bond Difference in electronegativity of more than 2.0 C, N, O, F the ability of an atom to attract toward itself the electrons in a chemical bond. mixing of two or more atomic orbitals to form a new set of hybrid orbitals less than 0.5 difference in electronegativity 3589 triple bond the sum of all polar bonds' dipole moments as vectors double bond
Match the key terms descriptions to the Balance Sheet and Income Statement classifications