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Chemistry 121 > Chapter Seven: Periodic Properties of the Elements > Flashcards

Chapter Seven: Periodic Properties of the Elements Flashcards

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1
Q

Mendeleev and Meyer both noted that similar chemical and physical properties recur periodically when the elements are arranged in order of increasing…

A

atomic weight

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2
Q

Moseley found that each element produced x-rays of a unique frequency and that the frequency generally increased as…increased

A

atomic mass

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3
Q

Moseley arranged the x-ray frequencies in order by assigning a unique whole number also known as a…to each element

A

Atomic Number

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4
Q

What law?
- The strength of the interaction between two electrical charges depends on the magnitudes of the charges and on the distance between them

A

Coulomb’s Law

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5
Q

The attractive force between an electron and the nucleus depends on the magnitude of the nuclear charge and on the average…between the nucleus and the electron

A

distance

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6
Q

The force increases as does nuclear charge, it decreases as the electron moves…from the nucleus

A

farther

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7
Q

In addition to the attraction of each electron to the nucleus, each electron experiences the repulsion due to other…

A

electrons

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8
Q

Each electron in a many-electron atom is…from the nucleus by the other electrons

A

screened

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9
Q

When an electron is screened by another electron, it experiences a net attraction…than it would experience in the absence of other electrons

A

smaller

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10
Q

What kind of charge?
- the net positive charge experienced by an electron in a many-electron atom; this charge is not the full nuclear charge because there is some shielding the nucleus by the other electrons in the atom

A

Effective Nuclear Charge

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11
Q

What kind of radius?
- The radius of an atom is defined by the distances separating it from other atoms to which it is chemically bonded

A

Bonding Atomic Radius

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12
Q

Within each group, bonding atomic radius tends to…from top to bottom

A

increase

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13
Q

Within each period, bonding atomic radius tends to…from left to right

A

decrease

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14
Q

The size of an ion depends on its nuclear charge, the number of…it possesses, and the orbitals that are most spatially extended from nucleus

A

electrons

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15
Q

What type of energy?
- minimum energy required to remove an electron from the ground state of the isolated gaseous atom or ion

A

Ionization Energy

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16
Q

The magnitude of the ionization energy tells us how much energy is required to…an electron

A

remove

17
Q

The greater the ionization energy, the more difficult it is to…an electron

A

remove

18
Q

Every element exhibits a large increase in ionization energy when the first of its inner shell electrons is…

A

removed

19
Q

Ionization generally…as we move left to right across a period

A

increases

20
Q

Ionization generally…as we move down any column in the periodic table

A

decreases

21
Q

In general, smaller atoms have…ionization energies

A

higher

22
Q

The energy needed to remove an electron from the outermost occupied shell depends on both the effective nuclear charge and the average…of the electron from the nucleus.

A

distance

23
Q

When electrons are removed from an atom to form a cation, they are always removed first from the occupied orbitals having the largest…

A

principal quantum number

24
Q

The first ionization energy of an atom is a measure of the energy change associated with removing an electron from the atom to form a…

A

cation

25
Q

All ionization energies for atoms are…

A

positive

26
Q

Energy must be…to remove an electron

A

absorbed

27
Q

What is affinity?
- the energy change that occurs when an electron is added to a gaseous atom or ion

A

Electron Affinity

28
Q

Ionization energy measures the energy change when an atom…an electron

A

loses

29
Q

Electron affinity measures the energy change when an atom…an electron

A

gains

30
Q

The greater the attraction between an atom and an added electron, the more…the atom’s electron affinity

A

negative

31
Q

Metals tend to have…ionization energies and therefore tend to form cations relatively easily

A

low

32
Q

Because of a nonmetal’s relatively large, negative electron affinities, nonmetals tend to…electrons when they react with metals

A

gain

33
Q

The first ionization energies of the alkaline earth metals are low but not as low as those of the…

A

Alkali Metals

34
Q

Alkaline earth metals are…reactive than their alkali metal neighbors

A

less

35
Q

The reactivity of hydrogen with nonmetals reflects its much greater tendency to hold on to its …

A

electron

36
Q

…has a great tendency to attract electrons from other elements

A

Oxygen

37
Q

Nonmetals melting and boiling points increase with increasing…

A

Atomic Number

Chemistry 121 (9 decks)

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