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Marine Chemistry > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

Dalton

A
  • published the first list of elements
  • Put them in atomic weight from lowest —> highest
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2
Q

Dobereiner

A
  • DIDN’T look at elements by weight
  • Created triads(groups of 3)
    *Problem: not all the elements were grouped/grouped improperly b/c it doesn’t work in every element
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3
Q

Bunsen

A
  • Invented the bunsen burner and spectroscope
    *This comes up with a new way to find and identify elements
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4
Q

Mendeleev

A
  • Published the 1st periodic table(1869)
  • Was missing a whole group(noble gasses)
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5
Q

Ramsey

A

Discovered noble gasses and made them a group(1900s)

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6
Q

Mosley

A
  • Created the atomic number
  • an’t have half a proton so nothing in between
    *Could only have 92 elements
  • His 1st periodic table(1913)
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7
Q

Berzelius

A
  • Glass-blowing guy
    *Coming up with accurate atomic weights
  • Wanted to organize the elements more accurately than Dalton
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8
Q

Newlands

A
  • Created the Law of Octaves
    *Every eighth element had similar properties
  • Concept is still used today(Periodic Law)
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9
Q

Periodic Law

A

a law saying the elements, when listed in order of their atomic numbers, will fall into recurring groups with other similar properties

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10
Q

Periodic Trend

A
  • are consistent changes in properties as you move across a period
    *period: horizontal groups on the table
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11
Q

Group Trend

A
  • are consistent changes in properties as you move down a group/family
    *group/family: vertical columns on table
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12
Q

Atomic radius

A
  • distance from the center of the nucleus → outer edge of electron cloud
    *More electrons/energy levels = bigger atom which means larger radius
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13
Q

Periodic/group trend for atomic radius

A

Radius decreases across periods
Radius increases down families/groups

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14
Q

Valence energy level

A
  • Outermost electrons will ALWAYS be in the s and p sublevels
  • MOST valence electrons you will ever see is 8(s(2) & p(6))
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15
Q

Valence electrons

A

electrons in the outermost energy level

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16
Q

Octet rule

A
  • 8 electrons in the outermost energy level (filled s & p sublevels) is the most stable electron configuration
  • Subgoals:
    *Full last-filled sublevel
    *Half-full last-filled sublevel
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16
Q

Ions

A

atoms or molecules that are not neutral

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17
Q

Ionization

A
  • process that results in forming an ion
    *Happens by adding or removing electrons
    *NO ion does ionization alone (paired process)
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18
Q

Ionization energy

A

measures how much energy it takes to remove an electron from an atom
*Higher IE → harder to steal from

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19
Q

1st, 2nd, 3rd, etc ionization energy

A

Energy needed to take the 1st, 2nd, 3rd, and etcetera electron

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19
Q

Electronegativity

A

is a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound.

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20
Q

Period/group trends for electronegativity

A

Increases across periods
Increases down groups/families

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21
Q

Key discoveries/work of scientists in order

A
  • Dalton published the 1st list of elements by order of atomic weight from lowest to highest
  • Berzelius, who was the glass-blowing guy. * Dobereiner observed elements by their chemical properties in triads
  • Bunsen invented the bunsen burner and spectroscope
    *Newlands created the Law of Octaves
  • Mendeleev published the first periodic table
  • Ramsey added the group known as the noble gasses
  • Moseley introduces the atomic number
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22
Q

First periodic table (how it was arranged, what was missing)

A
  • The first periodic table was arranged by atomic weight
  • The group known as the noble gasses was missing from the table.
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23
Q

Revised period table (how it was arranged, how it differed from first)

A
  • The revised periodic table was arranged by atomic number
  • It differed from the first table as there was also the noble gasses added to the table.
24
Q

Relationship between elements’ period/position and its electron configuration

A

Based on where the element is placed on the periodic table, it tells you the energy level, sublevel, spin, and more.
The energy level is numbered on the side. The d sublevel is (period - 1) where the f sub levels energy level is (period - 2).
The table is divided into sublevels.
The Groups 1 and 2 are in the s sublevel. Groups 3-12 are in the d sublevel.
Groups 13-18 are in the p sublevel.
The two rows below the periodic table are in the f sublevel.
As for the number of electrons, it depends on how far they are in the group.
SO if they are in the 5th column in their group, it would be 5. So, it shows the electron configuration of the element just by where it is.

25
Q

How/why hydrogen both fits in its group and doesn’t

A

Hydrogen fits in its group, alkali metals, because it has properties like the elements in group 1.

On the other hand, it does not fit because it can be placed in group 17, the halogen family. This is as it only needs 1 more electron to fill the valence electron shell.

26
Q

How/why helium both fits in its group and doesn’t

A

Helium fits in its group, noble gasses, because it has properties like them, a completely filled outermost shell.

On the other hand, it does not fit because its electron configuration ends in 1s^2 meaning it should actually be in Group 2.

27
Q

How/why certain d and f block elements’ configurations are exceptions (don’t need to know specific examples)

A

Certain d and f block elements’ configurations are exceptions because there is where the element is more/less stable because of how full their sublevels/energy levels are filled.

28
Q

Names of major groups on table

A
  • Alkali metals
  • Alkaline-earth metals
  • Transition metals
  • Oxygen family
  • Halogen family
  • Noble gasses.
29
Q

Properties for major groups on the table

A
  • Alkali metals are ductile/malleable, good electric/heat conductors, have a low melting point, and are very reactive.
  • Alkaline-earth metals are ductile/malleable, good electric/heat conductors, less reactive than alkali metals, and reactive.
  • Transition metals are malleable/ductile, good electric/heat conductors, higher melting point than groups 1 & 2, and are more brittle/harder than groups 1 & 2.
  • Oxygen family is made up of nonmetals/metalloids/metals, small atomic radii, and 6 valence electrons.
  • Halogen family is made up of all nonmetals, reactive, exist at solid/gas at room temperature, and dissolves.
  • Noble gasses are generally very unreactive, colorless, odorless, tasteless, and nonflammable.
30
Q

Trends for atomic number

A

Increases across periods
Increases down groups

31
Q

Trends for atomic mass

A

Increases across periods
Increases down groups

32
Q

Trends for atomic radius (and why)

A

Decreases across periods
Increases down groups

This is because of the increasing nuclear charge which makes the electrons have a stronger pull and shrink the radius.

33
Q

What sublevels will valence electrons always be in (and why)?

A

Valence electrons will always be in the s and p sublevels.
This is because this is the most amount of electrons there are eight and for it to be fully full, it would have to be either s(which fills up to two) or p(which fills up to six).

34
Q

What is the most stable configuration

A

When the electron valence shell is full.

35
Q

Trends for ionization energy (and why)

A

Increases across periods
Decreases down groups

This is because to remove an electron, it requires less energy when there are more electrons to take than when there are less electrons to take.

35
Q

2nd and 3rd most stable configurations

A

The second most stable configuration is when the last-filled sublevel is full.

The third most stable configuration is when the last-filled sublevel is half-filled.

36
Q

Why is second ionization energy higher?

A

The second ionization energy is higher because it requires a lot more energy to remove an electron from a split ion than it is from a neutral atom.

37
Q

And 3rd? And 4th?
Where will the big jump be?

A

The process continues.
There will be a big jump because once you lose two electrons, the atom becomes stable and it doesn’t want to lose anymore electrons.
This makes it even harder, requiring more energy/force to take more.

38
Q

Explain exceptions in ionization energy

A

When the electron configuration is different and because of Hund’s Rule.
It is close, but not exactly the right order for how ionization energy works like the alkaline-earth metals and noble gasses. Alkaline-earth metals usually have a higher IE.

39
Q

in developing his periodic table, Mendeleev listed on cards each element’s what?

A

name
atomic mass
properties

40
Q

which early scientist needed to learn to blow glass in order to make good enough tools to accurately measure atomic weights of the elements?

A

Berzelius

41
Q

Mendeleev predicted that the gaps in his periodic table represented what?

A

undiscovered elements

42
Q

the person whose work led to a periodic table based on increasing atomic number was who?

A

Moseley

43
Q

what is still accepted today and says that when elements are in order by atomic number, their properties will repeat every so many elements?

A

Law of Periodicity

44
Q

which group of elements was discovered by Sir William Ramsey?

A

noble gases

45
Q

which scientists was laughed at for suggesting properties of elements retreated in patterns every eight elements?

A

Newlands

46
Q

elements in group 18 have what level of radioactivity?

A

very low

47
Q

nonmetallic elements that react with most metals to form salts are what group and name?

A

Group 17, halogens

48
Q

in nature, the alkali metals are found only in compounds because of what?

A

they are very reactive elements

49
Q

for the s block, what is the energy level?

A

energy level = period

50
Q

for the p block, what is the energy level?

A

energy level = period

51
Q

for the d block, what is the energy level?

A

energy level = (period - 1)

52
Q

for the f block, what is the energy level?

A

energy level = (period - 2)

53
Q

for the s block, what is the period?

A

period = energy level

54
Q

for the p block, what is the period?

A

period = energy level

55
Q

for the d block, what is the period?

A

period = (energy level + 1)

56
Q

for the f block, what is the period?

A

period = (energy level + 2)

57
Q

the d and f blocks violate what principle?

A

Aufbau principle

58
Q

4 factors that impact ionization energy

A
  • number of protons: more protons = greater ionization energy
  • shielding effect: elements with valence electrons in higher energy levels have lower ionization energies
  • Radius: greater radius = lower ionization energy
  • sublevel: elements with half-full or full sublevel have greater ionization energies
59
Q

exceptions for ionization energy trends

A

Filled and half-filled sublevels can make element more stable, which makes IE higher

Marine Chemistry (11 decks)

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