Periodic Trends Flashcards
What scientist is credited for creating the periodic table?
- Demitri Mendeleev
- Published his version in 1869
- Periodic Law
There are _ vertical columns in the Periodic Table which are called _
- 18
- Groups
There are _ horizontal rows in the Periodic Table which are called _
- 7
- Periods
The majority of elements in the Periodic Table are _ which are mostly located on the _ side of the table
- Metals
- Left
The minority of elements in the Periodic Table are _ which are mostly located on the _ side of the table
- Nonmetals
- Right
There are 6 elements in the _ that are located in the boundary of metals and non-metals.
- Metalloids
How are the elements aranged on the periodic table?
They are arranged based on their similarities in electron configuration and they are grouped by their valence electrons.
(‘s’ block, ‘p’ block, ‘d’ block, ‘f’ block)
Which two groups of elements are in the ‘s’ block?
Alkali Metals and Alkaline Earth Metals
Group 1
- Alkali Metals
- 1 ve
- Lose 1
- Very Reactive
Group 2
- Alkaline Earth Metals
- 2ve
- Lose 2e
- Reactive
Groups 3-12
- Transition Metals
- Various # of ve
- Low Reactivity (Ex/ will react w/ oxygen in the air but slowly)
Group 16
- Oxygen Group
- 6ve
- Gain 2ve
- Reactive (like its counterpart in group 2)
Group 17
- Halogen (Means “Self-forming”)
- 7ve
- Gain 1ve
- Very Reactive (Nonmetal- Very reactive like counterpart in Group 1)
Group 18
- Nobel Gass
- 8ve
- Gain/Lose None
- Nearly Inert (means not generally reactive)
Octet Rule
Atoms with either gain or lose electrons to have a full outer shell of 8ve
Full Shell = Stability
Colombic Attraction Force
F = kq1q2/d2
k: Columbs constant
q1: Charge in first particle
q2: Charge in second particle
d: Distance between the two charged particles
The higher the _ the stonger the __
- Charge (# of protons)
- Attractive Force
The longer the _ the weaker the __
- Distance (from the nucleus to the ve)
- Attractive Force
Atomic Radius
- The average distance between the nucleus and the ve
- Usually measured as one-half distance between two nuclei of an element in its elemental form
Electronegativity
A measure of the ability of an atom to attract other electrons when the atom is part of a compound
Ionization Energy
The energy required to remove 1 electron from an atom
The # of _ is dominant
It _ across a period
Attractive Force _ from across a period
For elements in the same period
- Protons
- Increases
- Increases
Atomic Radius _ across a period
For elements in the same period
Decreases
Deaceases when there are less protons
Electronegativity _ across a period
For elements in the same period
Increases
Ionization Energy _ across a period
For elements in the same period
Increases
The _ between the nucleus and ve is dominant
It _ down a group
Attractive Force _ down a group
For elements in the same group
- Distance
- Increases
- Decreases
Atomic Radius _ down a group
For elements in the same group
increases
It increases bc/ there are more shells
Electronegativity _ down a group
For elements in the same group
Decreases
Ionization Energy _ down a group
For elements in the same group
Decreases
Electronegativity _ from left to right within a period and _ from top to bottom within a group
- Decreases
- Increases
As you move down a group, why does atomic radius increase?
It increases because there are more shells (energy levels)
Which has greater electronegativity: N or C?
N
What element has the lowest ionization energy in group 1 and why?
Cesium (Cs)
It is the lowest bc/ itd 1 ve is very far from the nucleus, so very little energy is needed to remove it
What element has the lowest ionization energy in group 1 and why?
Cesium (Cs)
It is the lowest bc/ itd 1 ve is very far from the nucleus, so very little energy is needed to remove it
What atom has the largest atomic radius in period 4?
K
The energy required to remove electrons
Ionization Energy
What element has the smallest ionization energy in period 5?
Rb
As you move across the periodic table, why do atoms tend to get smaller?
Because the atoms have more protons
The ability of an atom to attract other electrons
Electronegativity
What atom has the largets atomic radius in group 18?
Rn
As you move across the periodic table from left to right, the atomic radius . Why?
- Decreases
- This is bc/ the number of protons increses, so attraction to electrons increases
Elements in the same group will all have similar _
Properties
Group 3-12 is known as the _
Transition Metals
