Chapter 2: The Periodic Table Flashcards
The periodic table is organized based on increasing atomic ________.
number
the # of protons in an element
The periodic table is a visual representation of the periodic law, which states: the chemical and physical properties of the elements are dependent, in a periodic way, upon ________.
their atomic numbers
Groups contain elements that have the same electronic configuration in their ________ ________ and share similar chemical properties.
valence shell
The electrons in the valence shell, known as the ________ ________, are the farthest away from the nucleus and have the (greatest/least?) amount of potential energy.
valence electrons; greatest
held less tightly by the nucleus; can mingle
largest determinant of chemical reactivity
The Roman numeral above each group represents what?
The # of valence electrons that elements in that group have in their neutral state
also has an A or B to separate the elements into 2 larger classes
The A elements are known as the ________________ elements and they have their valence electrons in which orbitals?
representative; s or p subshells
The B elements are known as the ____________________ elements and include both the ________________ elements, which have valence electrons in which subshells?
They also include the ________________ and ________________ series, which have valence electrons in which subshells?
nonrepresentative; transition, s and d; lanthanide and actinide, s and f
________ are found on the left side and in the middle of the table. What 4 types do they include?
Metals;
1. Active
2. Transition
3. Lanthanide
4. Actinide
Metals are ________, meaning they can be hammered into shapes. They are also ________, meaning they can be pulled or drawn into wires.
malleable; ductile
Metals have:
1. (high/low?) effective nuclear charge
2. (high/low?) electronegativity
3. (small/large?) atomic radius
4. (small/large?) ionic radius
5. (high/low?) ionization energy
6. (high/low?) electron affinity.
- low
- low
- large
- small
- low
- low
allow metals to easily give up electrons
Many transition metals (Group B) elements have 2+ ________________ ________, which are charges when forming bonds with other atoms.
oxidation states
Valence electrons of metals are loosely held onto and are thus free to move, which makes metals good ________________ of electricity and heat.
conductors
Valence electrons of the active metals are found in the ____ subshell; those of the transition metals are found in the ____ and ____ subshells; and those of the lanthanide and actinide series elements are in the ____ and ____ subshells.
s; s and d; s and f
____________ are found predominantly on the upper right side of the periodic table. They are ____________ (texture) in the solid state and are not very lustrous, if at all.
Nonmetals; brittle
Nonmetals have:
1. (high/low?) ionization energy
2. (high/low?) electron affinity
3. (high/low?) electronegativity
4. (small/large?) atomic radii
5. (small/large?) ionic radii
They are not good conductors.
- high
- high
- high
- small
- large
do not easily give up e-‘s; less unified in chemical/physical properties
Separating the metals and nonmetals are a stair-step group of elements called the ________________, also known as semimetals. The electronegativities and ionization energies of the metalloids are inbetween metals and nonmetals.
metalloids
boron, silicon, germanium, arsenic, antimony, tellurium, polonium, astatine
The electrostatic attraction between the valence shell electrons and nucleus is known as ____________ ____________ ____________ - measure of net positive charge experienced by the outermost eleectrons.
effective nuclear charge
Zeff (decreases/increases?) from left to right. Why?
increases; adding a proton
Elements can gain/lose electrons in order to achieve a stable ____________, representative of the noble (inert) gas.
octet
there are exceptions!
________ ________ is 1/2 the distance between centers of 2 atoms of an element
atomic radius
Atomic radius (increases/decreases?) from left to right. Why?
decreases; electrons are added to the outermost shell with no additional shielding; increased positive charge means increased Zeff
Atomic radius (increases/decreases?) going down a group. Why?
increases; valence electrons are farther away with a virtually constant Zeff
________ ________ is the radius of a monatomic ion in an ionic crystal structure
ionic radius
For nonmetals close to the metalloid line, they need to (gain/lose?) more e- to achieve an octet, and thus have a (smaller/larger?) ionic radius.
gain; larger
For metals close to the metalloid line, they have more e- to (gain/lose?) to achieve an octet, and thus experience less drastic reduction in radius during ionization.
lose
____________ ________ is the energy required to remove highest energy electrons
ionization energy
Ionization energy is an ________________ process, as it requires input of heat
endothermic
The energy to remove the first e- is called the ________ IE.
first
An atom whose first valence e- has been removed is called a ________ cation (X+) and forms a divalent cation.
univalent
Elements in Groups 1 and 2 have such low ionization energies that they are called ________ metals. They do not exist in their neutral forms and are always found as ionic compounds.
active
The halogens (Group 17) typically (lose/gain?) an electron and are generally (cations/anions?).
gain; anions
A halogen gaining an electron to complete its octet is an ____________ process because it expels energy in the form of heat.
exothermic
________ ________ refers to the energy dissipated by a gaseous species when it gains an electron.
Electron affinity
essentially opposite from IE
Since electron affinity (gaining) is an exothermic process, ΔHrxn has a (negative/positive?) sign. However, electron affinity is reported as a (negative/positive?) number
negative; positive
The stronger the electrostatic pull between nucleus and VE is, the (greater/lesser?) the energy release will be when an atom gains an electron.
greater
Electron affinity (increases/decreases?) from left to right. Why?
Increases, because Zeff increases
Eleectron affinity (increases/decreases?) top to bottom, why?
decreases, because the valence shells are farther away
____________________ is the measure of attractive force that an atom exerts on an electron in a bond.
Electronegativity
Electronegativity is related to ________________ ________.
ionization energy
The lower the ionization energy, the (lower/higher?) the electronegativity is.
lower
The ________ metals (Group ____) possess most of the classic physical properties of metals, except that their densities are lower than those of other metals. They only have 1 loosely bound electron in their outermost shells.
alkali; 1
The alkali metals have very (low/high?) Zeff, and thus have the (largest/smallest?) atomic radii of all the elements.
low; largest
Alkali metals react readily with ____________, especially which group?
nonmetals; halogens
The ____________ ________ ________ have many properties of the alkali metals but have slightly (lower/higher?) Zeff and thus slightly (smaller/larger?) atomic radii.
alkaline earth metals; higher; smaller
The alkali metals usually form ________ cations.
univalent
The alkaline earth metals usually form ________ cations.
divalent
The ____________, which are Group ____, are a group of nonmetals and metalloids. They are not as reactive as halogens, but are crucial for normal biological functions. They each have 6 electrons in their valence shell and have (small/large?) atomic radii and (small/large?) ionic radii.
chalcogens; 16
small; large
most important are oxygen, sulfur, and selenium; the rest are metals
The ________, Group ____, are highly reactive nonmetals with 7 valenc e-. They have variabel physical properties and are desperate to complete their octet. VERY reactive with alkali and alkaline earth metals.
halogens, 17
Halogens are so reactive that they are not naturally found in their elemental state but rather as ions called ________ or as ________ molecules.
halides; diatomic
The ________ gases have extremely low boiling points and exist as gases at RT.
noble
The ____________ metals (Groups ____ to ____) are considered metals and have (high/low?) electron affinities, (high/low?) ionization energies, and (high/low?) electronegativities. They are hard and have high metling and boiling points. They tend to be malleable and good conductors since they have loosely held electrons that fill the d-orbitals.
transition; 3 to 12
Transition metals have different possible charged forms or ____________ ________ because they can lose different numbers of e- from the s and d orbitals in their valence shells.
oxidation states
causes many different ionic compounds to form
Metals in different oxidation states form complex ions that tend to associate in solution either with molecules of water and form ________________ ________ or with nonmetals.
hydration complexes
The ability to form hydration complexes contributes to the variable ________________ of certain transition metal-containing compounds.
solubility
e.g. AgCl can dissolve in ammonia but not water bc it forms a complex w/ it
The formation of complexes causes the ____-orbital to split into 2 energy sublevels This enables many complexes to absorb certain frequencies of light– those containing the precise amount of energy required to raise e- from the lower to higher energy d-orbitals.
d
The frequencies not absorbed (subtraction frequencies), give complexes their color
When we perceive an object as a particular color, it is because that color is not absorbed, but rather ____________ by the object.
reflected
If an object absorbs a given color of light and reflects all others, our brain mixes these ________________ ________________ and we perceive the ____________________ ________ of the frequency that was absorbed.
subtraction frequencies; complementary color
