Chemistry Periodic Properties

Question 1

The substance of this work is summarized in the ___, which states that the chemical properties of the elements are dependent, in a systematic way, upon their atomic numbers

Answer 1

periodic law

Question 2

Since [chemicals] share the same valence ___, elements within a group also share similar chemical properties

Answer 2

electron configuration

Question 3

The Roman numeral ___ each group represents the number of valence electrons

Answer 3

above

Question 4

The A elements are the ___, which have either s or p sublevels as their outermost orbitals

Answer 4

representative elements

Question 5

These representative elements are those in Groups IQ through VIIA, all of which have incompletely filled s or p subshells of the ___ principal number

Answer 5

highest

Question 6

The B elements are the ___, including the transition elements, which have partly filled d sublevels, and the lanthanide and actinide series, which have partly filled f sublevels

Answer 6

nonrepresentative elements

Question 7

The position of an element on the periodic table can be used to determine the ___ of valence electrons

Answer 7

electron configuration

Question 8

All elements seek to gain or lose valence electrons so as to achieve the ___, fully-filled formations possessed by the inert or noble gases of Group VIIIA

Answer 8

stable

Question 9

First, from left to right across a period, ___ are added one at a time and the electrons of the outermost shell experience an increasing degree of nuclear attraction, becoming closer and more tightly bound to the nucleus

Answer 9

protons

Question 10

When the electrons of the outermost shell experience an increasing degree of nuclear attraction, this net positive charge from the nucleus, as felt by an electron, is called the ___ (Zeff)

Answer 10

effective nuclear charge

Question 11

Second, from top to bottom down a given column, the outermost electrons become less tightly bound to the nucleus. This is because the number of filled principal energy levels (which shield the outermost electrons from attraction by the nucleus) ___ downward within each group

Answer 11

increases

Question 12

Taken together, these trends show that Zeff is at a maximum for elements in the top-right of the table and at a minimum for those in the bottom-left and help explain elemental properties such as ___, ionization potential, electron affinity, and electronegativity

Answer 12

atomic radius

Question 13

The atomic radius of an element is equal to one-half the distance between the centers of two atoms of that element that are just barely ___ each other

Answer 13

touching

Question 14

In general, the atomic radius decreases across a period from left to right and increases ___ a given group; the atoms with the largest atomic radii will be located at the bottom of groups and toward the left of the table (Group IA)

Answer 14

down

Question 15

From left to right across a ___, electrons are added one at a time to the outer energy shell

Answer 15

period

Question 16

Electrons within the same shell do not ___ one another from the attractive pull of protons

Answer 16

shield

Question 17

Therefore, since the number of protons is also increasing from left to right across a period, the effective nuclear charge (Zeff) ___ as well

Answer 17

increases

Question 18

The greater the positive charge experienced by the valence electrons (the larger the Zeff), the closer those electrons are pulled toward the ___ and the smaller the atomic radius

Answer 18

nucleus

Question 19

From top to bottom down a ___, the number of electrons and filled electron shells increase

Answer 19

group

Question 20

Although the number of ___ electrons within a group remains the same, these valence electrons will be found farther from the nucleus as they are in progressively larger energy shells

Answer 20

valence

Question 21

As ___ are found in progressively larger energy shells, Zeff will become smaller with distance, so valence electrons in higher energy shells will feel less pull from the nucleus

Answer 21

electrons

Question 22

Also, with more electrons comes increased ___ from the additional negative (-) charges. Thus, the atomic radii will increase

Answer 22

repulsion

Question 23

The ___ is the radius of a cation or an anion

Answer 23

ionic radius

Question 24

In most situations, cations (positive ions) will be smaller than corresponding neutral ___ since possessing fewer electrons leads to less repulsion among the remaining electrons

Answer 24

atoms

Question 25

The ___ (IE) is the energy required to completely remove an electron from a gaseous atom or ion

Answer 25

ionization energy

Question 26

Removing an ___ from an atom always requires an input of energy and is endothermic

Answer 26

electron

Question 27

The first ionization energy is the energy required to remove one valence electron from the parent atom, the second ionization energy is the ___ needed to remove a second valence electron from the univalent ion to form the divalent ion, and so on

Answer 27

energy

Question 28

However, if the removal of a second ___ from an element would give it a fully-filled or half-filled valence shell, then the second ionization energy would be lower than the first since atoms are more stable when the valence shell is fully or half-filled

Answer 28

electron

Question 29

___ (EA) is the energy change that occurs when an electron is added to a gaseous atom, an it represents the ease with which the atom can accept an electron

Answer 29

electron affinity

Question 30

The ___ the Zeff, the greater the electron affinity will be

Answer 30

higher

Question 31

The more common sign convention for ___ states that a positive electron affinity value represents energy release when an electron is added to an atom; the other states that a negative electron affinity represents a release of energy

Answer 31

electron affinity

Question 32

Group IIA elements, or alkaline-earth metals, have low ___ affinity values

Answer 32

electron

Question 33

Alkaline earth metals are relatively stable because their s ___ is filled

Answer 33

subshell

Question 34

Group VIIA elements, or halogens, have high electron affinities because the addition of an electron to the atom results in completely filled shell, which represents a ___ electron configuration

Answer 34

stable

Question 35

Achieving the stable octet (halogens) involves a release of energy, and the strong attraction of the ___ for the electron leads to a high change in energy

Answer 35

nucleus

Question 36

The Group VIIIA elements (noble gases) have electron affinities on the order of ___ because they already possess full shells and cannot readily accept electrons

Answer 36

zero

Question 37

Electronegativity is a measure of the ___ an atom has for electrons in a chemical bond

Answer 37

attraction

Question 38

The greater an atom’s ___, the greater its attraction for bonding electrons

Answer 38

electronegativity

Question 39

___ are related to effective nuclear charge: elements with low Zeff will have low electronegativities because their nuclei do not attract electrons strongly, while elements with high Zeff will have high electronegativities because of the strong pull the nucleus has on electrons

Answer 39

electronegativities

Question 40

Therefore, electronegativity increases from left to right across ___ and decreases from to top bottom down a group

Answer 40

periods

Question 41

Metals are shiny solids (except for mercury) at ___ and generally have high melting points and densities

Answer 41

room temperature

Question 42

Metals have the characteristic ability to ___ without breaking

Answer 42

deformed

Question 43

The ability of a metal to be hammered into ___ is called malleability, and the ability to be drawn into wires is called ductility

Answer 43

wires

Question 44

Many of the characteristic properties of ___, such as large atomic radius, low ionization energy, and low electronegativity, are due to the fact that the few electrons in the valence shell of a metal atom can easily be removed

Answer 44

metals

Question 45

Because the valence electrons can move freely, metals are good conductors of heat and ___

Answer 45

electricity

Question 46

Groups IA and IIA represent the most ___ metals

Answer 46

reactive

Question 47

The transition elements, are ___ that have partially filed d orbitals

Answer 47

metals

Question 48

The nonmetals are located on the upper right side of the periodic table and are separated from the metals by a line cutting diagonally through the region of the ___ table containing elements with partially filled p orbitals

Answer 48

periodic

Question 49

The ___ and ionization energies of metalloids lie between those of metals and nonmetals; therefore, these elements possess characteristics of both those classes

Answer 49

electronegativities

Question 50

___ are made up of cations and anions, where a cation is a positive ion and an anion is a negative ion

Answer 50

ionic compounds

Question 51

An older, but still commonly used, \_\_\_is to add the ending -ous or -ic to the root of the Latin name of the element to represent the ions with lesser or greater charge, respectively.
Fe2+  - Ferrous
Fe3+ - Ferric
Cu+ - Cuprous
Cu2+ - Cupric

Answer 51

method

Question 52

Monatomic \_\_\_ are named by dropping the ending of the elemental name and adding -ide.
H- - Hydride
F- - Fluoride
O2- - Oxide
S2- - Sulfide
N3- - Nitride
P3- - Phosphide

Answer 52

anions

Question 53

Many polyatomic anions contain oxygen and are ___ called oxyanions

Answer 53

therefore

Question 54

When an \_\_\_ forms two oxyanions, the name of the one with less oxygen ends in -ite and the one with more oxygen ends in -ate.
NO2- - Nitrite
NO3- - Nitrate
SO32- - Sulfite
SO43- Sulfate

Answer 54

element

Question 55

When the series of \_\_\_ contains four oxyanions, prefixes are also used. Hypo- and per- are used o indicate less oxygen and more oxygen, respectively
ClO- - Hypochlorite
ClO2 - - Chlorite
ClO3 - - Chlorate
ClO4 - Perchlorate

Answer 55

oxyanions

Question 56

Polyatomic ___ often gain one or more H+ ions to form anions of lower charge. The resulting ions are named by adding the word hydrogen or dihydrogen to the front of the anion’s name. An older method uses the prefix bi- to indicate the addition of a single hydrogen ion.
HCO3 - Hydrogen carbonate or bicarbonate
HSO4 - Hydrogen sulfate or bisulfate
H2PO4 - Dihydrogen phosphate

Answer 56

anions

Question 57

All ___ in a given group tend to form monatomic ions with the same charge

Answer 57

elements

Question 58

Though other main group ___ follow the trend of each element in a group tending to form monatomic ions with the same charge, the intermediate electronegativity of such elements (which makes them less likely to form ionic compounds) and the transition from metallic to nonmetallic character further complicates the picture

Answer 58

elements

Question 59

___ can also form the hydride ion (H-), which is far too reactive to exist in water. In this respect, hydrogen resembles the halogens in that it only requires one additional electron to reach the next noble gas configuration

Answer 59

hydrogen

Question 60

The alkali metals have only one loosely bound electron in their outermost ___, giving them the largest atomic radii of all the elements in their respective periods

Answer 60

shell

Question 61

___ metallic properties and high reactivity are due to their low ionization energies; they easily lose their valence electron to form univalent cations, allowing them to easily form +1 cations

Answer 61

alkali metals

Question 62

The alkaline earth metals are the elements of Group IIA and also possess many characteristically ___ properties

Answer 62

metallic

Question 63

The ___ have two electrons in their outer shell and have smaller atomic radii than the alkali metals

Answer 63

alkaline earth metals

Question 64

___ have low electronegativities and positive electron affinities

Answer 64

alkaline earths

Question 65

The family containing carbon, Group IVA, exhibits a wide range of characteristics and includes a ___(C), metalloids (Si and Ge), and metals (Sn and Pb)

Answer 65

nonmetal

Question 66

Although Group IVA do not share many physical properties, they do all have 2 electrons in their ___ p subshells, leading to a configuration that is distant from that of a noble gas

Answer 66

outermost

Question 67

The 2 ___ in outermost shell make Group IVA tend not to form ions (which would need to be +4 or -4 to reach noble gas configuration)

Answer 67

electrons

Question 68

Carbon participates in electron sharing; it usually is most stable with four ___ bonds

Answer 68

covalent

Question 69

___ also commonly holds a positive charge in organic reactions, making several nitrogen-containing compounds good bases

Answer 69

nitrogen

Question 70

Halogens chemical properties are more uniform: The ___ of halogens are very high, and they are particularly reactive toward alkali metals and alkaline earths, which “want” to donate electrons to the halogens to form stable ionic crystals

Answer 70

electronegativities

Question 71

___ are completely nonreactive because they each have a complete valence shell, which is an energetically favored arrangement

Answer 71

noble gases

Question 72

Because noble gases each have a complete ___, this gives them no tendency to gain or lose electrons, high ionization energies, and no electronegativities - they possess low boiling points and are gases at room temperature

Answer 72

valence shell

Question 73

Chemically, Groups IB to VIIIB (transition metals) have low ionization ___ and may exist in a variety of positively charged forms or oxidation states

Answer 73

energies

Question 74

___ are capable of losing various numbers of electrons from the s and d orbitals of their valence shells

Answer 74

transition metals

Question 75

The ___ of complexes causes the d orbitals to be split into two energy sublevels. This enables many of the complexes to absorb certain frequencies of light - those containing the precise amount of energy required to raise electrons from the lower to the higher d sublevel. The frequencies not absorbed - known as subtraction frequencies - give the complexes their characteristic colors

Answer 75

formation

Question 76

For transition ___, the dissolved ions can form complex ions either with molecules of water (hydration complexes) or with nonmetals, forming highly colored solutions and compounds (e.g., CuSO4 with 5H2O yielding chalcanthite)

Answer 76

metals