The Periodic Table Flashcards
The modern periodic table is organized based on increasing _____ _____.
Atomic number
Rows of elements on the periodic table are referred to as ______; columns are called ______.
Periods; groups (or families)
The A elements are known as the _______ elements and include groups IA through VIIIA. The elements in these groups have their valence electrons in the orbitals of either s or p subshells.
Representative
The B elements are known as the ________ elements and include both the transition elements, which have valence electrons in the s and d subshells, and the lanthanide and actinide series, which have valence electrons in the s and f subshells.
Nonrepresentative
Metals are found on the left side and in the middle of the periodic table. List some characteristics of metals.
- Lustrous (shiny) solids (except for Hg at room temp.)
- Generally, high melting points and densities
- Malleable
- Ductile
- Good conductors of heat and electricity (due to their electrons being free to move)
True or false: Metals easily give up electrons, which leads to characteristics such as low ionization energy and low electron affinity.
True
Nonmetals are found on the upper right side of the periodic table. What are some characteristics of nonmetals?
- Brittle and show little or no metallic luster
- High ionization energies, electron affinities, and electronegativities
- Poor conductors of heat and electricity
(All of these characteristics are manifestations of the inability of nonmetals to easily give up electrons.)
(HIGH YIELD) The electrostatic attraction between the valence shell electrons and the nucleus is known as the _____ _____ _____, a measure of the net positive charge experienced by the outermost electrons.
Effective nuclear charge (Z sub eff)
(HIGH YIELD) For elements in the same period, does the effective nuclear charge increase or decrease from left to right?
Increase
(HIGH YIELD) From top to bottom in a group, does the effective nuclear charge increase or decrease, or is it held constant?
It is held constant because the increased shielding created by the inner shell electrons cancels the increased positivity of the nucleus.
(HIGH YIELD) The _____ _____ of an atom is equal to half the distance between the centers of two atoms of an element that are briefly in contact with each other.
Atomic radius
(HIGH YIELD) Describe how atomic radii change as you move across and down the periodic table.
Atomic radii decrease as you move from left to right across a period; they increase as you move from top to bottom down a group.
(HIGH YIELD) _______ _______ is the energy required to remove an electron from a gaseous species.
Ionization energy (IE)
(HIGH YIELD) Is the removal of an electron from an atom an exothermic or endothermic process?
Endothermic
(HIGH YIELD) Describe how ionization energy changes as you move across and down the periodic table.
Ionization energy increases from left to right and decreases from top to bottom (because the electrons are held less tightly by the nucleus as the principal quantum number increases).
(HIGH YIELD) True or false: The second ionization energy is always greater than the first ionization energy.
True. Electrons are being removed from increasingly cationic (positive) species.
(HIGH YIELD) The active metals are found in what groups?
Groups IA and IIA (Groups 1 and 2)
(HIGH YIELD) Which group of elements is the least likely to give up electrons?
Group VIIIA (Group 18) elements, or the Noble gases. They are among the elements with the highest ionization energies.
(HIGH YIELD) When an atom acquires an electron, is this an endothermic or exothermic process?
Exothermic
(HIGH YIELD) Describe how electron affinity changes as you move across and down the periodic table.
Electron affinity increases from left to right and decreases from top to bottom.
(HIGH YIELD) ________ is a measure of the attractive force than an atom will exert on an electron in a chemical bond.
Electronegativity. It increases from left to right and decreases from top to bottom.
List the common names for each of the following groups on the periodic table: Group 1, Group 2, Group 16, Group 17, Group 18, and Groups 3-12
Group 1 - Alkali Metals Group 2 - Alkaline Earth Metals Group 16 - Chalcogens Group 17 - Halogens Group 18 - Noble Gases Groups 3 - 12: Transition Metals
One of the unique properties of the transition metals is that many of them can have different possible charged forms or ______ ______ because they are capable of losing different numbers of electrons from the s- and d-orbitals in their valence shells.
Oxidation states
Antimony is used in some antiparasitic medications. What type of element is antimony (Sb)?
Metalloid
Which property of metals explains why they are used in making wires that conduct electricity?
Metals have valence electrons that can move freely.
