Module 2 content Flashcards

Question

Molecule shapes and bond angles/pairs

Answer 1

Linear= regions, 180 degrees Non-linear= 2 bonded pairs, 2 lone pairs, 104.5 degrees Pyramidal= 3 bonded, 1 lone, 107 degrees Trigonal planar= 3 regions, 120 degrees Tetrahedral= 4 bonded, 109.5 degrees Octahedral= 6 regions, 90 degrees

Answer 2

The ability of an atom to attract the bonding electron in a covalent bond

Answer 3

Increases across and up the table A higher Pauling scale value= higher electronegativity

Answer 4

The bonded electron pair is shared unequally between bonding atoms Bonded atoms have different electronegativity values= polar covalent bond

Answer 5

The more electronegative atom has a greater attraction for the bonded pair The more electronegative atom has a delta - charge and the other a delta positive Exists in polar covalent bonds If dipoles in a molecule act in opposite directions and exactly oppose one another they will cancel out and make a non-polar molecule

Answer 6

Induced dipole-dipole interactions (London)= weakest Permanent dipole-dipole Hydrogen bonding= strongest In covalent bonding Responsible for physical properties

Answer 7

Weak and exist between all molecules 1) Movement of e- produces changing dipole 2) At any time, an instantaneous dipole will exist but it's position constantly shifts 3) This dipole induces a dipole on the next molecule 4) This induced dipole then induces further dipoles on next molecules which then attract another

Answer 8

Temporary More e- in each molecule= larger instantaneous/induced dipoles,=greater induced dipole interactions= stronger forces between molecules= higher bp

Answer 9

Same forces as in a permanent dipole Non-polar substances= only London forces Polar= London forces& permanent dipoles= extra energy needed to break permanent dipole= higher bp

Answer 10

Molecules held by weak IMFs Atoms are bonded strongly by Covalent bonds Low bp (only need to break IMFs) Non conductors= no mobile charged particles, no circuit can be complete

Answer 11

Non-polar substances are soluble in non-polar solutes: IMFs form between molecules and solvent Weaken the IMFs in the simple molecular lattice, break and then compound dissolves Are insoluble in polar solvents: The IMFs in the polar solvent are too strong to be broken by the interactions

Answer 12

May dissolve in polar solvents as molecules can attract each other The solubility depends on the dipole strength Compounds w/ polar and non-polar parts can dissolve in both Carbon chain= non-polar

Answer 13

Permanent dipole-dipole interaction between molecules w/ an electronegative atom w/ a lone pair or H-O, H-N,H-F Acts between lone pair on an electronegative atom and H on another

Answer 14

Solid ice is less dense than water= H bonds hold water molecules apart in open lattice, molecules are further apart in ice, less dense and floats Relatively high bp= H bonds and London forces, more energy needed to break H bonds, only when water boils are bonds completely broken

Module 2 content Flashcards

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