periodic trends

first ionization energy

-amount of energy required to remove the most loosely bound electron from a gaseous atom in its group state -they are always endothermic and IE values are always positive

ionization energy (IE)

-energy required to remove an electron -elements are usually in a gaseous state -Fluorine is most IE -if two elements are equal distances apart, unlike in electronegativity, you cannot tell which has higher IE

exceptions to electron affinity

-group 1 to 2 (one is higher) -group 14 to 15 (14 is higher)

electronegativity

-how well an element can attract electrons -F is the most electronegative atoms -noble gases are not electronegative -one that is higher up is more electronegative if two elements are equidistance from Florine

electronegativity trend

-increases left to right -increases bottom to top

electron affinity trend

-increases left to right and bottom to top

ions size....

-increases the more negative it is

atomic radii trend

-increases top to bottom and right to left -decreases across period

atomic radii

-one half the distance b/n the nuclei

isoelectronic

-same electron configuration -same number of electrons

successive IE

-the 2nd IE is always greater than the first and will continue to increase from there -there will be a huge jump in IE after you take the last one from a shell bc then you will start taking electrons from noble gas configuration

electron affinity (EA)

-the energy change for the process of adding an electron to a gaseous atom to form an anion -can be endo or exothermic -F is the highest -noble gases will have lower EA

types of trends

1. size (radii) of atoms and ions 2. ionization energies 3. electron affinities 4. electronegativity

For an atom of carbon, which ionization will exhibit a very large increase in the energy relative to the preceding ionization?

5th, There are four valence electrons in an atom of carbon. The 5th ionization will require a very large increase in the energy relative to the preceding ionization

Which of the following series of elements has nearly the same atomic radii? A) Ti, V, Cr, Mn B) Mg, Ca, Sr, Ba C) B, Si, As, Te D) Cl, Br, I, At E) K, Ca, Ga, Ge

A) Ti, V, Cr, Mn The atomic radius increases as you move down the periodic table and to the left. Ti, V, Cr, and Mn are next to each other in the same row and do not vary much in atomic radii.

Which of the following series of isoelectronic ions correctly lists the ions in order of increasing size (i.e., smallest to largest)?

Ca²⁺ < K⁺ < Cl⁻ < P³⁻ For isoelectronic species, anions will be larger than cations. Ions can be further ranked by considering their charges. The greater the negative charge, the larger the size. The greater the positive charge, the smaller the size.

Which of the following is true concerning successive ionizations of an atom and its ions?

Each successive ionization requires increasing amounts of energy -Each successive ionization of an atom and its ions requires increasing amounts of energy to remove the electrons.

What element is theoretically the largest of all on the periodic table?

Francium (Fr) -Atomic radius increases as you move down the periodic table and to the left. Francium is the furthest down and to the left of this group and would be predicted to to be the largest element of the whole periodic table.

Under which process does an atom demonstrate the largest increase in size in one step?

Gaining its first electron to become a -1 anion -Anions are larger than the neutral atom from which they derived. Generally the change in size is greatest when an atom gains/loses its first electron. Subsequent changes in overall charge lead to smaller changes

Which of the following radii comparisons is correct? A) N³⁻ < N B) Ti⁴⁺ > Ti³⁺ C) In³⁺ < In⁺ D) C⁴⁺ > C⁴⁻ E) As³⁻ < As³⁺

In³⁺ < In⁺ Cations are always smaller than the neutral atom from which it is derived. Anions are always larger than the neutral atom from which it is derived. Therefore, the smaller ion in a pair will be the one with fewer electrons.

Which periodic trend quantifies the amount of energy required to remove an electron from a neutral, gaseous atom?

Ionization Energy

Which of the following metals would be expected to have the smallest atomic radius?

The atomic radius increases as you move down the periodic table and to the left. Tantalum is the furthest to the right of this list and nearer the top and it would be expected to have the smallest atomic radius.

In which direction along the periodic table does thermal conductivity generally increase?

Thermal conductivity generally increases as you move left across a period.

ion size from largest to smallest

anions (-), neutral, cations (+)

exceptions to ionization energy

comparing groups 2 to 13, 2 has greater ionization energy despite trend -comparing groups 15 to 16 group 15 has higher ionization energy despite trend

removing ______________ electrons requires more energy than ___________ electrons

core, valence

more neg ion=

decrease zeff and larger radius

ionization energy trend

increases left to right and bottom to top

metallic character

increases right to left and top to bottom

removing an electron from a cation is more difficult than removing an electron from a ________________

neutral atom

Which of the following elements is the most electropositive? -F -Cl -P

p -Phosphorus is the least electronegative of this group and therefore the most electropositive.

more positive ion=

smaller radius