Periodic Trends Flashcards
What did Moseley’s periodic table look like?
Elements were arranged by atomic number.
What did Mendeleev’s periodic table look like?
Elements were arranged by similar properties and increasing atomic mass.
What is the arrangement of atomic radii on a periodic table?
Atomic radii increases as you go down a group, and decreases from left to right across a period.
What is effective nuclear charge?
The positive charge on a nucleus.
What happens the ionic radii on a periodic table?
It increases down a group, and increases from right to left across a period, which includes a trade off from metal to nonmetal.
What is a cation?
A positive ion
What is an anion?
A negative ion
What ions do metals form?
Cations
What ions to nonmetals form?
Anions
Where are cations found?
Groups 1, 2 and 3.
Where are anions found?
Groups 5, 6 and 7.
What does atomic radii estimate?
Size
What is ionization energy?
Increase from left to right on period and increase up a group. Energy used to remove electrons and forms ions.
What is special about noble gases?
They don’t lose energy easily, and since they’re nonmetals, they have higher ionization.
What is second ionization energy?
Removal of additional electrons from an atom.
What is electronegativity?
The measure of ability of atom to attract electron. Increases right a period and up a group.
What is a halogen?
An element in group 17.
What is a transitional metal?
All elements in groups 3-12 in d block.
What is an alkali metal?
Elements in group 1
What is an alkali earth metal?
Elements in group 2 except of Be.
What is the shielding affect?
Describes attraction between atom and nucleus. Decreases down groups, constant across periods.
How does nuclear charge determine atomic radius and what is it similar too?
It’s equal to atomic number, and the larger the atomic radius the smaller the nuclear charge and vise-versus for smaller atomic radius.
How is a cation formed and what does this process lead too?
It’s formed by loss of electrons which leads to a decrease in atomic radius.
What is the affect of cations on electrons?
Cations draw electrons towards nucleus.
