Bonding Flashcards
What is Hund’s rule?
Electrons enter orbitals with parallel spins first (until all orbitals contain one electron)
What does the last electron placed in an electron configuration represent?
The quantum number.
What is the difference between abbreviated and unabbreviated electron configurations?
Unabbreviated shows the entire configuration for the element, while abbreviated shows the last noble gas (as a placeholder) and the rest of the configuration only.
Abbreviated electron configuration for cobalt? (Just an example, no need to memorize)
[Ar] 4s^2 3d^7
Argon is the last noble gas before cobalt, so it acts as a placeholder.
Where are valence electrons found and what is their significance?
They are found in the outermost energy level. They determine how reactive an element is.
What is the octet rule?
8 total electrons in the valence energy level represents a stable electron configuration/arrangement.
Noble gases are also called…
inert gases.
Why are elements in the noble gases (group 18) stable?
They have eight electrons in the outermost energy level. They follow the octet rule.
The noble gas electron configuration always ends in…Does this configuration represent a stable or unstable element?
Configuration ends in __s^2__p^6.
s2p6 represents a stable element/configuration.
How can octet structure be achieved by an element that is not a noble gas (already stable)?
Valence electrons can be added or removed in the valence energy level to achieve octet structure (8 valence electrons, or s2p6 configuration).
Elements in group 1 have how many valence electrons?
1.
What is the significance if an element has four valence electrons?
The atom can either gain four electrons or lose four electrons to obtain octet structure.
What does oxidation state show?
Charge. Ex: Li+ is the common oxidation state for lithium.
What does the Lewis Dot diagram show?
The element’s valence electrons.
Lanthanides and actinides are also known as…
Inner transition elements/metals.
The most active metals are located…
In group 1 (1A) (Alkali metals)
The most active nonmetals are located…
In group 17 (7A) (Halogens)
What is the most active halogen?
Fluorine.
Is an anion larger or smaller than its parent atom?
Larger.
Is a cation larger or smaller than its parent atom?
Smaller.
An element with both metallic and nonmetallic properties is called a…
metalloid or semi-metal.
Elements in a group have the same number of…
Valence electrons.
Elements in a period have the same number of…
Electron shells/energy levels.
The majority of the elements on the periodic table are…(metals or nonmetals)
Metals.
As you go down a group, elements generally become (more or less) metallic.
More metallic.
What does a colored ion indicate?
A transition metal.
Group 1 elements are called…
How many valence electrons do they have?
What is their most common oxidation state?
Alkali metals. They have 1 valence electron. Their most common oxidation state is 1+.
Group 2 elements are called…
How many valence electrons do they have?
What is their most common oxidation state?
Alkaline earth metals. They have 2 valence electrons. Their most common oxidation state is 2+.
Groups 3-12 elements are called…
Transition metals.
Group 13 (3A) valence electrons? Oxidation state?
3 valence electrons. Oxidation state: 3+.
Group 14 (4A) valence electrons? Oxidation state?
4 valence electrons. Oxidation state: 4+/-.
Group 15 (5A) valence electrons? Oxidation state?
5 valence electrons. Oxidation state: 3-.
Group 16 (6A) valence electrons? Oxidation state?
6 valence electrons. Oxidation state: 2-.
Group 17 (7A) valence electrons? Oxidation state?
7 valence electrons. Oxidation state: 1-.
Group 18 (8A) valence electrons? Oxidation state?
8 valence electrons: Oxidation state: 0, because they are stable and non-reactive.
On the periodic table, where is the s-sublevel found?
Groups 1 and 2: alkali metals and alkaline earth metals. Also helium.
On the periodic table, where is the p-sublevel found?
Groups 13-18, excluding helium.
On the periodic table, where is the d-sublevel found?
Groups 3-12: transition metals.
On the periodic table, where is the f-sublevel found?
Lanthanide and actinide series.
After 4s on the periodic table, next in that row is:
3d. (NOT 4d!)
After 2s on the periodic table, next comes:
2p.
The f-sublevel contains only two rows of elements: The lanthanides and actinides. These two rows represent:
4f and 5f.
In each row of the “d” block there are only 10 elements. Why?
This is because the d sublevel can hold at maximum 10 electrons. The number of elements in each row of a certain sublevel corresponds to the maximum number of electrons that sublevel can hold.
What is the effect of distance between protons and electrons on force of attraction?
As distance between two oppositely charged particles (protons and electrons) increases, force of attraction decreases.
What is coulombic attraction?
Attraction between two oppositely charged particles.
As you move down a group, how does distance between valence electrons and nucleus change?
As you move down a group, distance between the valence electrons and the nucleus increases (because you are adding energy levels).
As you move down a group, how does force of attraction between valence electrons and nucleus change?
As you move down a group, force of attraction decreases because distance between electrons and protons increases.
How does the number of protons in the nucleus affect attractive force between electrons and protons?
As number of protons increases, attractive force increases.
For each proton added, how much does force increase?
Each proton increases force of attraction by 2.30 x 10^ -8 N if distance is .10 nm
Does force of attraction change when electrons are added?
Slightly, because electrons repel each other, but not by much. Each electron still gets approximately the full force of the nucleus. (Ex: If there are 3 protons and 3 electrons, each electron receives 6.90 x 10^-8.)
What is atomic radius?
A way to express the size of an atom
How does one find atomic radius?
Atomic radius= 1/2 the distance between the nuclei of 2 identical atoms that are bonded together in a diatomic molecule.