General Chemistry Ch. 2 Flashcards
The periodic table is organized by increasing ____
atomic number/number of protons
Define the Periodic Law
The chemical and physical properties of elements are dependent upon atomic numbers
Group A elements have valence electrons in the ___ subshell(s)
S or p
Define representative elements
Groups IA-VIIIA that have valence electrons in s or p subshells
Define non representative elements
Transition elements that have valence electrons in s and d subshells and lanthanide and actinide series that have valence electrons in s and f subshells
Group B have elements in the ___ subshell(s)
s and d or s and f
Transition elements have electrons in their ___ subshell(s)
s and d
The actinide and lanthanide series have electrons in their ___ subshell(s)
s and f
____ are non representative elements
Transition metals, lanthanide series, actinide series
___ are representative elements
Groups IA-VIIIA
Metals have ___ densities
High
Metals have ___ melting points
High
Metals have ____ effective nuclear charge
Low
Metals have ___ electronegativity
Low
Metals have ____ atomic radii
Large
Metals have ___ ionic radii
Small
Metals have ___ ionization energy
Low
Metals have ___ electron affinity
Low
Most transition metals have ___ or more oxidation states
2
Active metals have valence electrons in the ___ subshell(s)
S
Transition metals have valence electrons in the ___ subshell(s)
s and d
The lanthanide and actinide series have electrons in the ___ subshell(s)
s and f
Nonmetals have ___ ionization energy
High
Nonmetals have ____electron affinities
High
Nonmetals have ___ electronegativity
High
Nonmetals have ___ atomic radii
Small
Nonmetals have ___ ionic radii
Large
List the metalloids
- Boron (B)
- Silicon (Si)
- Germanium (Ge)
- Arsenic (As)
- Antimony (Sb)
- Tellurium (Te)
- Polonium (Po)
- Astatine (At)
Define and give the symbol for effective nuclear charge
Z (sub) eff: the electrostatic attraction between valence shell electrons and the nucleus. The measure of net positive charge experienced by outermost electrons
The effective nuclear charge increases as you go ___ to ___ across the periodic table
Left to right
The effective nuclear charge is the same among elements of the same ___
Group
The atomic radius increases as you go ___ and ___ on the periodic table
Down and left
Nonmetals close to the metalloid line have (larger/smaller) ionic radii than those closer to the noble gases
Larger
Metals near the metalloid line have (larger/smaller) ionic radii than other metals
Smaller
Define ionization energy/potential
The energy needed to remove an electron from a gaseous species
Ionization energy increases as you go ___ and ___ on the periodic table
To the right and up
The energy to remove the first electron is (greater/less than) the energy needed to remove subsequent electrons
Less than
Define first ionization energy
The energy needed to remove the first electron
Groups __ and __ have low ionization energies
IA and IIA
Groups ___ and ___ do not exist neutral forms and are found as ionic compounds, minerals, or ores
IA and IIA
In ionic form, group ___ exists as anions
VIIA
Group __ are halogens
VIIA
Define electron affinity
The energy dissipated by a gaseous species when it gains an electron
Electron affinity increases as you go ___ and ___ across the periodic table
To the right and up
Define electronegativity
The attractive force that an atom exerts on an electron in a chemical bond
Lower ionization corresponds to ___ electronegativity
Lower
Noble gases have ___ electronegativity
Negligible
Electronegativity increases as you go ___ and ___ across the periodic table
Right and up
The ____ scale quantifies electronegativity
Pauling
What group is the alkali metals
Group IA
The alkali metals have ___ densities
Lower
Alkali metals have __ electron(s) in the outer shell
1
The alkali metals have ___ atomic radii
Large
Alkali metals have ___ ionization energy
Low
Alkali metals have __ electron affinity
Low
Alkali metals have ___ electronegativity
Low
Alkali metals highly react with ___
Nonmetals
What group is the alkaline earth metals?
Group IIA
Alkaline earth metals have __ effective nuclear charge and __ atomic radii
Larger; smaller
Alkaline earth metals have __ electron(s) in their valence shell
2
Alkali metals lose their electron(s) to form ___
Univalent cations
Alkaline earth metals lose their electron(s) to form ___
Divalent cations
What group are chalcogens?
Group VIA
Chalcogens have __ valence electron(s)
6
Lighter chalcogens are __ whereas denser chalcogens are __
Nontoxic; toxic
What group are halogens?
Group VIIA
Halogens have __ electron(s)
7
What state are halogens?
Gaseous, liquid, or solid
Halogens have __ electronegativity
High
Halogens have __ electron affinity
High
Halogens easily bind to __
Alkali metals and alkaline earth metals
Halogens aren’t found in their __ state, but rather found in the __ or __ state
Elemental; diatomic or halide/ionic
What group are inert gases?
Group VIIIA
Inert gases are __ reactive (highly/moderately/minimally)
Minimally
Inert gases have ___ ionization energy
High
Inert gases have __ electronegativity
No
Inert gases have __ valence electron(s)
8
Inert gases have __ boiling points
Low
What group are transition elements found?
IB-VIIIV (3-12)
Transition elements are ___
Metals
Transition elements have ___ electron affinities
Low
Transition elements have ___ ionization energies
Low
Transition elements have ___ electronegativities
Low
Transition elements have ___ melting points
High
Transition elements have ___ boiling points
High
