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Chem 1610 > Chapter 7 > Flashcards

Chapter 7 Flashcards

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1
Q

what is Zeff?

A

effective nuclear charge

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2
Q

what is the formula for Zeff?

A

Zeff = Z - P

Z = atomic number
P = # of core electrons

e. g. Zeff(Al) = 13 - 10 = 3
e. g. Zeff(Si) 14 - 10 = 4

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3
Q

what is the trend for Zeff?

A

increases to the right

decreases going down a group

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4
Q

what is the trend for atom size?

A

size increases down a group

generallyy decreases from left to right

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5
Q

explain the trend for atom size

A

group: b/c same outer shell electron configuration and increase in n (orbital size)
family: b/c Zeff increases and inner electrons shield outer electrons from the full positive charge of the nucleus

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6
Q

which is bigger, cation or anion?

A

anions are bigger in atomic radius, cations are smaller in atomic radius

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7
Q

how do you determine size for ions?

A

if they all have the same number of electrons, the atom with the most protons has the highest Zeff —> the higher the Zeff the smaller the radius

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8
Q

how do ions move in an electronic device?

A

from cathode to anode when charging

when using electronics they discharge from anode to cathode

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9
Q

what is the first ionization energy?

A

the energy required to remove the highest energy electron from neutral gaseous atoms

the energy is POSITIVE

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10
Q

second ionization energy

A

second ionization energy: I2: always requires more energy than I1 because removing a negative particle from a positive ion

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11
Q

IE trend

A

IE decreases down a group because: atomic radii increases down a group and +/- attraction decreases with greater distance: electrons are further away from the nucleus and aren’t as tightly bound

IE generallyyyy increase across a period from left to right because electrons are held tightly: Zeff is greater

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12
Q

exceptions to the IE trend?

A

elements with filled s or half filled p subshells have higher IE than expected

  • Be > B: Be is 2s and B is 2p. electrons in 2p are shielded from the positive charge of the nucleus by electrons in the 2s orbital. electron in the 2s orbital are not effective in shielding each other
  • N > O
  • Zn, Cd, Hg
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13
Q

what is electron affinity?

A

the energy given off when adding an electron to a gaseous atom

  • not a well established trend
  • second EA always requires energy (endothermic) b/c a second electron must be forced onto an already negatively charged ion
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14
Q

metallic character trend

A

metallic character increase from right to left and top to bottom

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15
Q

why do metals form cations?

A

low IE

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16
Q

why do nonmetals usually form anions?

A

high IE and EA

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17
Q

nonmetals

A

form molecules

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18
Q

metals

A

form ionic compounds

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19
Q

oxides of metals

A

basic

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20
Q

oxides of nonmetals

A

acidic

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21
Q

metalloids

A

IE are too high to form cations

EA too negative to form anions

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22
Q

group 1A

A
  • alkali metals
  • soft
  • low density
  • form M+ ions
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23
Q

what are the most important alkali metals?

A

Li, K, Na
- occur in oceans, salt beds, and minerals
- preparation of free metals by reduction:
LiCl —> 2Li(s) + Cl2(g)

24
Q

what happens when alkali metals react with oxygen?

A
  • react with oxygen: most be stored in oil because they redly react with the air
  • oxides form with Li
  • peroxides form with Na
  • superoxides form with K, Rb, and Cs
25
Q

what happens when alkali metals react with water?

A

Li: moderate
Na: rapid
K: in flames
Rb and Cs: explode

26
Q

group 2A

A
  • alkali earth metals
  • harder
  • more dense
  • less reactive than Group 1A due to smaller size and increase in Zeff
  • form M+2 ions
27
Q

what are the most important alkali earth metals?

A

Mg, Ca (most abundant too)

  • occur as silicates, carbonates, and sulfates
  • magnesium is even found in the ocean
28
Q

what happens when alkali earth metals react with oxygen and water?

A

react less vigorously with oxygen and water than 1A

CaCO3(s) + heat -> CaO(s) + CO2(g)
CaO(s) + H2O(l) + Ca+2(aq) + 2OH-(aq)
Mg+2(aq) + 2OH-(aq) —> Mg(OH)2(s)
Mg(OH)2 + 2HCl(aq) —> MgCL2(s) + 2H2O(l)

29
Q

hydrogen

A
  • diatomic (H2)
  • odorless, colorless gas
  • 3 isotopes
  • 1s1: high IE so shares e- in covalent bonds like H2O
  • can also gain an electron (ionic bond like in NaH)
30
Q

what are the isotopes of hydrogen?

A

1H: hydrogen: 99.9%
2H: deuterium: .01%
3H: tritium: radioactive

31
Q

oxygen

A
  • diatomic (O2)
  • odorless, colorless gas
  • 21% air composed of oxygen - isolated from air
  • has allotropes
  • has 3 ions
32
Q

what are allotropes? what are oxygens allotropes?

A

same element but different compounds

O2 and O3(ozone)
3O2(g) + 284.6kJ —> 2O3(g) + O2(g)

33
Q

what are the 3 ions of oxygen?

A 
- oxide (O^-2): C/S/P vs Li/Ca/Al
     C: CO vs. CO2
     P: P2O10 vs. P4O6(acidic)
     S: so2 vs SO3
- peroxide(O2^-2): unstable 
     2H2O(aq) —> 2H2O(l) + O2(g) + 196.1 kJ
- superoxide (O2^-1): rescue masks
34
Q

sulfur

A

S8

  • a ring
  • yellow solid
  • makes acidic solution
  • S^-2(sulfide): S(s) + O2(g) —> SO2(g) —> SO3(g)
35
Q

nitrogen

A
  • diatomic (N2)
  • odorless, colorless gas
  • 78% of the air - isolated from the air
36
Q

what is the range of charge for the ions of nitrogen?

A

-3 to +5

find oxidation state of nitrogen
N2O5
NH3, N2H4
N2O, NO, NO2, N2O4, HNO2, HNO3

37
Q

phosphorous

A 
P4
- strained Td solid
- formed with: rock + sand + coke: 
     Ca3(PO4)2 + SiO2 + C —>  CaSiO3 + CO + P
- 3 allotropes
38
Q

what are the allotropes of phosphorous?

A

white, red, black

39
Q

halogens

A
  • high EA….X-

- you always make an acid when you combine a nonmetal with water: Cl2(g) + H2O(l) —> 2HCl(g)

40
Q

nobel gases

A
  • monoatomic
  • full s and p shells
  • high IE
  • thought to be unreactive until 1962: XeF2, XeF4, XeF6
41
Q

why does IE of nobel gases decrease as you move down a group?

A

decreases as you move down b/c IE is taking an electron away and the atom gets bigger as you go down so it’s easier to take an electron

42
Q

carbon

A
  • solid
  • covalent bonding
  • CO, CO2, H2CO3 (buffer in our blood)
  • hydrocarbons
  • 2 forms
43
Q

what are the 2 forms of carbon?

A

crystalline and amorphous forms

44
Q

silicon

A
  • solid
  • prepared with sand and coke
  • semiconductors that power our devices
  • SiO2
  • silicates: SiO4^-2 (asbestos)
  • silicones - (SiOR2)n - caulk, implants
45
Q

SiO2

A

sand and window glass

46
Q

boron

A
  • octet exception
  • rocket fuel
  • B2H6 + O2 —> B2O3 + H2O + 2030kJ (HC Brown 1979 Nobel Prize)
47
Q

among the nonmetallic elements, the change in atomic radius in moving one place left or right in a row is smaller than the change in moving up or down. explain.

A

when moving up or down you add an entire shell because n increases. when you move left or right only zeff varies which played a minor roll in comparison

48
Q

explain any difference in the orders of atomic and ionic size when it comes to anions and cations of atoms

A

anions are larger than cations. secondly, these ions are isoelectronic so when looking at size, the atom w/ the highest atomic # and most protons is the smallest because Zeff is larger

49
Q

Na2O + H2O –>

A

NaOH

50
Q

BaO + H2O –>

A

Ba(OH)2

51
Q

N2O5 + H2O –>

A

HNO3

52
Q

SO3 + H2O–>

A

H2SO4

53
Q

HNO3 + Sc2O3 –>

A

Sc(NO3)3 + H2O

54
Q

what is needed to make a basic solution?

A

H2O

55
Q

in born haber, make sure to double BOTH Hf and IE/EA if needed (like in MgCl2)

A

DONT FORGET

56
Q

what do you always make when you combine a nonmetal with water?

A

an acid

Cl + H2O –> HCl

Chem 1610 (7 decks)

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