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