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Chemistry 111 > Final > Flashcards

Final Flashcards

1
Q

alpha radiation

A

charge +2 and 4 amu —- new element formed has mass no. lower by 4 and atomic no. lower by 2

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2
Q

beta radiation

A

one additional p in the nuc. and at. no. incs. by 1 (mass doesn’t change

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3
Q

y radn

A

no charge or mass

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4
Q

positron emission

A

at. no. decs. by 1

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5
Q

Group 1

A

alkali metals

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6
Q

group 2

A

alkaline earth metals

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7
Q

group 16

A

chalcogens

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8
Q

group 17

A

halogens

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9
Q

group 18

A

noble gases

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10
Q

metals

A

conductor

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11
Q

nonmentals

A

nonconductors

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12
Q

metalloids

A

between metal/nonmental

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13
Q

weighted average

A

(mass1 x abundance1) x (mass2 x abundance2) x (mass3 x abundance3)

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14
Q

Avogadro’s number

A

6.022 x 10^23

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15
Q

jj thompson

A

atoms made up of 3 subatomic particles

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16
Q

robert Millikan

A

determined mass and charge of electron

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17
Q

thomson’s plum-pudding model

A

electrons distributed throughtout diffuse, positively charged sphere

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18
Q

Rutherfords

A

positively charged gold foil, some particles deflected, electrons negatively charged

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19
Q

nuclear model of atom

A

central psoitively charged nuc. where nearly all mass is concentrated, and is comprised of positively charged ‘
s and neutral n’s around which negatively charged e’s circulate in nearly empty space

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20
Q

isotope

A

atoms of an element containing same number of protons but diff number of neutrons

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21
Q

intensive properties

A

independent of amount of substance present (density)

22
Q

extensive properties

A

dependent upon amount of substance (mass, length, volume)

23
Q

density

A

d=m/v

24
Q

two nonmetals form compound

A
  1. first word is name of first element
  2. change word ending of second word to -ide
  3. use prefixes unless first element is mono
25
Q

Electronegativity

A

increases from left to right and decreases going down

26
Q

less than or equal to 0.4

A

nonpolar covalent

27
Q

0.4 - 2.0

A

polar covalent

28
Q

greater than or equal to 2.0

A

ionic

29
Q

formal charge

A

(number of valence e’s) - [number of unshared e’s + 1/2(number of e’s in bonding pairs)]

30
Q

why do we need to draw the Lewis struc of a molecule before predicting its geometry

A

to determin how many lone pairs are on a central atom and where they are

31
Q

Explain why C-O bonds are more polar than H-S bonds

A

carbon and oxygen are more electronegative than hydrogen-sulfur (closer to F so more polar)

32
Q

electron affinity

A

typically increase with increasing atomic number, becomes more negative across a row
hallogens have most EA
noble gases have low EA bc stable

33
Q

Lattice energy

A

energy required to break up the lattice *smallest distance (size) = stronger LE

34
Q

attractions between molecules that hold them together, these forces are electrical in origin and result from the mutual attraction of unlike charges or the mutual repulsion of like charges

A

intermolecular forces

35
Q

hydrocarbons

A

organic compound containing carbon and hydrogen only

36
Q

alkenes

A

hydrocarbons with double bond C’s (C=C)

37
Q

Alkynes

A

hydrocarbons with C to C triple bond

38
Q

alkanes

A

hydrocarbon with single bonds to carbon

39
Q

intermolecular force between atoms or nonpolar molecules caused by presence of temporary dipoles

A

london dispersion forces

40
Q

london dispersion forces

A

increase down table

41
Q

strength of dipole-dipole forces

A

increases going up table

42
Q

the result of electrical interactions between dipoles on neighboring molecules

A

dipole dipole forces

43
Q

as dipole force increases…

A

intermolecular forces increase

44
Q

as molar mass increases

A

boiling point increases (LDF increases)

45
Q

properties of water

A
  1. b.p. of H2O elements
  2. H2O has high delta H vaporization
  3. density of ice less than density of liquid H2O
46
Q

attractive forces between ion and molecules

A

ion-dipole interactions

47
Q

as strength of intermolecular forces increase, viscosity increases

A

as temp increases, viscosity decreases (disrupting IMF)

48
Q

triple point

A

temp and pressure of all three phases coexist

49
Q

critical point

A

specific temp and pressure where liquid and gas phase have same density and are indistinguishable

50
Q

supercritical fluid

A

substance in state that is above temp and pressure of critical point

Chemistry 111 (9 decks)

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