Ch 25 Flashcards

1
Q

Who published the first version of his periodic table, in which elements were ordered via atomic weight?

A

Dmitri Mendeleev

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2
Q

Henry Moseley organized elements based on

A

Atomic number

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3
Q

The periodic law states that

A

Chemical properties of the elements depend on their atomic number

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4
Q

There are seven periods (rows), each representing

A

The principal quantum numbers n = 1 to n = 7

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5
Q

Groups (columns) represent elements that have the same

A

Electronic configuration in their valence shell

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6
Q

The A elements are the

A

Representative elements

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7
Q

Representative elements have what as their outermost orbitals

A

Sublevels s and p

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8
Q

The B elements are non representative and fill orbitals

A

S, d, and maybe f

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9
Q

Transition elements have partly filled

A

D sublevels

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10
Q

Partly filled f levels are found in

A

Lanthanide and actinide series

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11
Q

From left to right across a period (row), the electrons experience

A

Nuclear attraction, becoming closer to the nucleus

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12
Q

What is the effective nuclear charge?

A

Net positive charge of the nucleus felt on electron

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13
Q

Down a given column, the outermost electrons become

A

Less tightly bound to the nucleus

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14
Q

The number of filled principal energy levels change how as you go downwards a group?

A

Increases

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15
Q

Zeff (effective nuclear charge) is at a maximum for elements

A

In the top-right of the table

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16
Q

Zeff (effective nuclear charge) is at a minimum for elements

A

In the bottom-left

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17
Q

Atomic radius increases

A

Right to left, and from up to down

18
Q

The atoms with the largest radii will be located

A

Bottom of the groups and towards the left of the table

19
Q

Something that affects the size of an electron will also

A

Change radius of an atom

20
Q

The addition of protons increases from left to right across a period, leading to an increase in

A

Zeff (effective nuclear charge)

21
Q

Valence electrons in higher energy shells will feel less pull become

A

Zeff becomes smaller with distance

22
Q

What will be smaller, cations or anions?

A

Cations

23
Q

What is Ionization energy?

A

Energy required to remove an electron from a gaseous atom or ion

24
Q

Removing an electron requires an input of energy, meaning it is

A

Endothermic

25
Q

What it the first ionization energy?

A

Energy required to remove one valence electron from the parent atom

26
Q

What is the second ionization energy?

A

Energy needed to remove a second valence electron

27
Q

Ionization energy increases from

A

Left to right across a period, and going up a group

28
Q

Why do group 1a elements have low ionization energies?

A

The loss of an electron results in the formation of a stable, noble-gas configuration

29
Q

What is the energy change that occurs when an electron is added to a gaseous atom, representing the ease by which atom can accept the electron?

A

Electron affinity

30
Q

How is electron affinity when Zeff is high

A

Electron affinity is great

31
Q

A negative electron affinity represents

A

Energy release

32
Q

Why do Group VIIA elements, or halogens, have high electron affinities?

A

The addition of an electron results in a completely filled shell

33
Q

What is the measure of the attraction an atom has for electrons in a chemical bond

A

Electronegativity

34
Q

The greater an atom’s electronegativity, the greater its

A

Attraction for bonding electrons

35
Q

The most common electronegativity scale is the

A

Pauling electronegativity scale, ranging from 0.7 to 4.0

36
Q

Electronegativities are related to

A

Effective nuclear charge

37
Q

Electronegativity increases from

A

Left to right, and down to up

38
Q

What are the three categories of elements?

A

Metals, nonmetals, and semimetals

39
Q

Metals have properties like:

A
  • Large atomic radius
  • Low ionization energy
  • Low electronegativity
  • Malleable
40
Q

What is the ability to be drawn into wires called

A

Ductility