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