Electron configuration and chemical periodicity

Question 1

In 1869, * independently proposed the
*:
• When the * are arranged in order of *, certain sets of properties recur periodically

Answer 1

Dmitri Mendeleev and Lothar Meyer
periodic law
elements, increasing atomic mass,

Question 2

In *, Dmitri Mendeleev and Lothar Meyer independently proposed the
periodic law:
• When the elements are arranged in order of increasing atomic mass, certain sets
of * recur * .

Answer 2

1869

properties, periodically

Question 3

Splitting of Energy Levels

• The * nuclear charge Z * orbital energy by * nucleus-electron attractions.

Answer 3

higher, lowers, increasing

Question 4

Splitting of Energy Levels

• The higher * lowers * by increasing *

Answer 4

nuclear charge Z, orbital energy, nucleus-electron attractions.

Question 5

An additional electron raises the * due to *.
• Electrons in outer orbitals (higher n) are higher in energy because inner electrons * them from * (effective nuclear charge, Zeff)

Answer 5

orbital energy, electron-electron repulsions

shield, nuclear charge

Question 6

An additional electron * the orbital energy due to electron-electron repulsions.
• Electrons in * (higher n) are higher in energy because * shield them from nuclear charge (*)

Answer 6

raises
outer orbitals
inner electrons
effective nuclear charge, Zeff

Question 7

Electrons that have a * probability distribution near the nucleus (*) have * energy. Thus, an * (shell) is split into * (subshell) energies: s < p < d < f .

Answer 7

finite, penetration, lower

energy level, sublevel

Question 8

Electrons that have a * (penetration) have lower energy. Thus, an energy level () is split into
sublevel () energies: s < p < d < f .

Answer 8

finite probability distribution near the nucleus

shell, subshell

Question 9

The * of an atom is a designation of how electrons are

* among various orbitals in principal shells and subshells.

Answer 9

electron configuration, distributed

Question 10

The electron configuration of an atom is a * of how electrons are distributed among various * in *

Answer 10

designation
orbitals
principal shells and subshells

Question 11

Electrons occupy * in a way that * the energy of the atom.

Answer 11

orbitals, minimizes

Question 12

Pauli exclusion principle. No two electrons can have * set of * . An orbital can hold a maximum of * electrons, and they must have * spins.

Answer 12

the same, four quantum numbers (n, l,ml ,ms)

two, opposite

Question 13

Hund’s rule. For orbitals of identical energy (*), electrons initially occupy these orbitals *.

Answer 13

degenerate orbitals, singly (before pairing up)

Question 14

The Aufbau Principle: electrons fill orbitals starting at the * before filling * (e.g. 1s before 2s).

Answer 14

lowest available (possible) energy states, 
higher states

Question 15

The * states that electrons fill orbitals starting at the lowest available (possible) energy states before filling higher states (e.g. 1s before 2s). It is also called *

Answer 15

Aufbau Principle

Building-Up Principle

Question 16

The order in which these orbitals are filled is given by the * rule, which states
that given two orbitals, the one which has a higher n value but a lower (n + l) value
is considered to be of a * .
• Also called the * rule or the Klechkowski rule.

Answer 16

(n + l)
lower energy level
Madelung

Question 17

The order in which these orbitals are filled is given by the (n + l) rule, which states
that given two orbitals, the one which has a * value but a * value
is considered to be of a lower energy level.
• Also called the Madelung rule or the * rule.

Answer 17

higher n, lower (n + l)

Klechkowski

Question 18

Hund’s Rule states that for degenerate orbitals, the * is attained when the number of electrons with the * spin is maximized.
also called Hund’s Rule of *.

Answer 18

lowest energy, same

Maximum Multiplicity

Question 19

The * refers to the periodic recurrence of certain * when the elements are considered in terms of *

Answer 19

periodic law
physical and chemical properties
increasing atomic number.

Question 20

The periodic law refers to the * of certain physical and chemical properties when the * are considered in terms of increasing atomic number.

Answer 20

periodic recurrence, elements

Question 21

The * is an arrangement of the elements, by *, in which elements with similar physical and chemical properties are grouped together
in *

Answer 21

periodic table, atomic number

vertical columns

Question 22

The periodic table is an * of the elements, by atomic number, in which elements with * are grouped together
in vertical columns

Answer 22

arrangement,

similar physical and chemical properties

Question 23

A * is a vertical column of elements in the periodic table. Members of a group have *.

Answer 23

group, similar properties

Question 24

A * is a horizontal row of the periodic table. All members of a period have atoms with *

Answer 24

period

the same highest principal quantum number.

Question 25

The first two groups–the s block–and the last six groups–the p block–together constitute the * elements. Because they come between the s block and the p block, the d block elements are known as the *.

Answer 25

main-group | transition elements

Question 26

The first two groups–the * –and the last six groups–the *–together constitute the main-group elements. Because they come between the s block and the p block, the * elements are known as the transition elements.

Answer 26

s block, p block | d block

Question 27

The f block elements, sometimes called the * The 15 elements following barium (Z = 56) are called the *, and the 15 following radon (Z = 88) are called the *

Answer 27

inner transition elements, lanthanides actinides

Question 28

The * elements, sometimes called the inner transition elements, The 15 elements following * are called the lanthanides, and the 15 following * are called the actinides

Answer 28

f block barium (Z = 56) radon (Z = 88)

Question 29

The atomic radius of an element is a measure of the *, usually the distance from the * to the *

Answer 29

size of the atom | nucleus, boundary of the surrounding cloud of electrons

Question 30

* is one-half the distance between the centers of two atoms that are bonded covalently. It is the atomic radius associated with an element in its covalent compounds. * is the radius of a spherical ion. It is the atomic radius associated with an element in its ionic compounds. * is one-half the distance between the centers of adjacent atoms in a solid metal.

Answer 30

Covalent radius Ionic radius Metallic radius

Question 31

The * are strictly hard sphere radii measured using atomic distances in closest packed *. • solid sample of a noble gas

Answer 31

van der Waals radii, | crystals

Question 32

The atomic radius tends to * as one progresses across a period from left to right • because the effective nuclear charge (Zeff) *, thereby * the orbiting electrons and lessening the radius

Answer 32

decrease | increases, attracting

Question 33

The * tends to decrease as one progresses across a period from left to right • because the * (Zeff) increases, thereby attracting the orbiting electrons and * the radius

Answer 33

atomic radius, effective nuclear charge | lessening

Question 34

The atomic radius usually * while going down a group | • due to the addition of a new *

Answer 34

``` increases energy level (shell). ```

Question 35

Cations are * than the atoms from which they are formed. | • For isoelectronic cations, the more * the ionic charge, the * the ionic radius.

Answer 35

smaller | positive, smaller

Question 36

Anions are * than the atoms from which they are formed. | • For isoelectronic anions, the more * the charge, the * the ionic radius.

Answer 36

larger | negative, larger

Question 37

The ionization energy, I, is the quantity of energy a gaseous atom must * to be able to * an electron

Answer 37

absorb, expel

Question 38

The * is the energy required to remove the * electron from a * atom.

Answer 38

first ionization energy I1 | most loosely held, gaseous

Question 39

The second ionization energy I2 is the energy required to remove an electron from a *.

Answer 39

gaseous unipositive ion

Question 40

Ionization energies * as atomic radii *. • IE * down a group. • IE * across a period.

Answer 40

decrease, increase | decreases, increases

Question 41

Electron affinity is the energy * associated with the * of an electron by a * atom.

Answer 41

change, gain, neutral gaseous

Question 42

The smaller atoms to the right of the periodic table (e.g., group 17) tend to have * electron affinities. • EAs tend to become * in progressing toward the bottom of a group, with the notable exception of the second-period members of groups 15, 16, and 17 (namely, N, O, and F). • Some atoms have no tendency to gain an electron, such as the noble gases where electrons have to enter the next shell, and groups * where the electrons have to enter an empty p subshell, etc.

Answer 42

large, negative less negative 2 and 12

Question 43

Electronegativity (EN) is a measure of the * of an atom to * electrons towards itself in the context of a chemical bond.

Answer 43

ability, attract

Question 44

EN is related to IE and EA. In 1934, * developed an approach where EN = *

Answer 44

Robert S. Mulliken | IE − EA2

Question 45

As one moves from left to right across a period in the periodic table, the electronegativity * • due to the stronger attraction that the atoms obtain as the * increases

Answer 45

increases, nuclear charge

Question 46

Moving bf down a group, the electronegativity * • due to the longer * between the nucleus and the valence electron shell, thereby * the attraction.

Answer 46

decreases distance decreasing

Question 47

In general, EN is * related to atomic size.

Answer 47

inversely

Question 48

An important property related to the electron configurations of atoms and ions is their * in a magnetic field. A spinning electron is an electric charge in *, which induces a *

Answer 48

behavior | motion, magnetic field

Question 49

• A diamagnetic substance has all its electrons * and the individual magnetic effects cancel out. It is slightly repelled by a magnetic field. • A paramagnetic substance has one or more * electrons in its atoms or molecules and the individual magnetic effects do not cancel out. It is attracted into a magnetic field.

Answer 49

paired | unpaired

Question 50

A metal is an element whose atoms have * numbers of electrons in the * electronic shell. Removal of an electron(s) from a metal atom occurs without great difficulty, producing *.

Answer 50

small, outermost | a positive ion (cation)

Question 51

Metals generally have a * appearance, are *, and are | able to *.

Answer 51

lustrous malleable and ductile conduct heat and electricity

Question 52

A nonmetal is an element whose atoms tend to gain small numbers of electrons to form * with the electron configuration of a *. Nonmetals are mostly *, *(bromine), or * solids and are very * conductors of heat and electricity.

Answer 52

``` negative ions (anions), noble gas ``` gases, liquid, low melting point poor

Question 53

A * is an element that may display both metallic and nonmetallic properties under the appropriate conditions.

Answer 53

metalloid

Question 54

Metallic property * across a period with * in number of valence electrons, as well as * in atomic radius, and it * down the group with increase in the *

Answer 54

decreases increase, decrease increases number of shells and atomic radius.