Unit 3 - Periodic Table Flashcards
(32 cards)
In what group(s) are the alkali metals found?
Group 1
In what group(s) are the alkaline earth metals found?
Group 2
In what group(s) are the transition metals found?
Group 3 - 12
In what group(s) are the halogens found?
Group 17
In what group(s) are the noble gases found?
Group 18
What are the properties of alkali metals?
Highly reactive with water, Soft and shiny, Conduct electricity
What are the properties of alkaline earth metals?
Reactive with water, Shiny, Conduct electricity
What are the properties of transition metals?
Shiny, Ductile, Malleable, Generally unreactive
What are the properties of halogens?
Brittle, Poor conductors, Reactive with alkali and alkaline earth metals
What are the properties of noble gases?
Extremely unreactive, Gaseous at room temperature, Poor conductors, Brittle
How many valence electrons do elements group 1 have?
1 valence electron
How many valence electrons do elements group 2 have?
2 valence electrons
How many valence electrons do elements group 17 have?
7 valence electrons
How many valence electrons do elements group 18 have?
8 valence electrons
What is the periodic trend: Atomic Radius
How we measure atoms, defined as half the distance between two nuclei of the same element.
How does Atomic Radius change as you go down a group and across a period?
It increases down a group and decreases across a period due to electron shielding, where the electrons not in the valence shell block the electrostatic force from the nucleus.
How is atomic radius affected when an atom becomes an ion?
DECREASES for cations and INCREASES for anions.
What is the periodic trend: Reactivity
Measures if an element will react with another substance and how fast it does so.
How does Reactivity change as you go down Group 1 (metals)? How does it change as you move down Group 17 (non-metals)? How does it change across the periodic table
For metals, it increases down a group and decreases across a period. For non-metals, it decreases down the group and increases across a period
What is the periodic trend: Ionization Energy
the amount of energy required to pull an electron away from the nucleus.
How does Ionization Energy change as you move down a group? How does it change as you move across the periodic table?
It decreases down the group and increases across the period.
How does Ionization Energy connect to valence electrons and the formation of chemical bonds?
Generally the less valence electrons there are, the lower the ionization energy. It is easier to remove one or two electrons than 6 or 7, even to complete the octet. The movement of electrons from one atom to another causes chemical bonding.
What is the octet rule?
states that all electrons want a full valence shell (usually eight electrons).
What do atoms do to reach a full octet?
They will lose or gain electrons until they have the full shell.
