Chapter 6 Flashcards
Antoine Lavoisier
Compiled a list of 23 known elements.
John Newlands
Noticed that when elements are arranged by increasing atomic mass, their properties repeated every 8 elements. The law of octaves. It was not accepted because it did not work for all known elements. People thought the musical analogy was unscientific so they rejected it.
Lothar Meyer
Demonstrated a connection between atomic mass and elemental properties in the same year as Mendeleev, but is given less credit because he published his organization scheme later, and Mendeleev predicted properties about elements yet to be discovered.
Dmitri Mendeleev
Noticed that when elements are arranged by increasing atomic mass, there was a periodic pattern in their properties. By arranging the elements in order of increasing atomic mass into columns with similar properties, Mendeleev organized the elements into the first periodic table.
Which elements’ properties was Mendeleev able to predict?
Scandium, Gallium, Germanium
Henry Moseley
Solved the problems with Mendeleev’s table by arranging the elements by atomic number.
Periodic Law
There is a periodic repetition of chemical and physical properties of the elements when they are arranged by increasing atomic number.
(T/F) Groups/Families are Horizontal
Vertical
(T/F) Periods are Horizontal
True
Representative Elements
Groups 1-2 and 13-18. Their last filled electron is a valence electron. They have a wide range of chemical and physical properties
Transition Elements
Groups 3-12, which have electrons that have just been filled in the D or F orbitals.
What are the 3 main classifications for the elements?
Metals, nonmetals, metalloids/semi-metals
Metals
Elements that are generally shiny when smooth and clean, solid at room temperature, and good conductors of heat and electricity.
(T/F) Metals are malleable but not ductile
Metals are malleable (Can be pounded into thin sheets) AND ductile (Can be stretched into wires)
(T/F) All group B elements are metal
True
What is the one element on the left side of the periodic table that is not a metal?
Hydrogen
1A/1 (Except for H)
Alkali metals
2A/2
Alkaline Earth metals
What are the two sets of inner transition metals?
The lanthanide and the actinide series
Does the Lanthanide series come first or the Actinide series?
The Lanthanide series comes first. It is in period 6 while the Actinides are in period 7.
Transition metals
Elements in groups 3-12.
(T/F) Elements from the actinide series are used to make phosphors
Elements from the LANTHINIDE series are used to make phosphors (substances that emit light when struck by electrons)
What is in the upper right hand corner of the periodic table?
Nonmetals
Nonmetalls are elements that…
Are generally gasses or brittle, dull looking solids. They are poor conductors of heat and electricity.
(T/F) There are no liquid nonmetals at room temperature
Bromine is the only nonmetal that is a liquid at room temperature.
7A/17
Halogens (Highly reactive)
8A/18
Noble gasses
Metalloids
Elements with physical and chemical properties of both metals and nonmetals.
What two metalloids are used in computer chips and solar cells?
Silicon and Germanium
Atoms in the same group have the same properties because ____
They have the same number of valence electrons. For example, in group 1A, all the valence shells have a configuration of _s1
The outermost energy level that an atom has electrons in is also the same as the atom’s ______ on the periodic table
Period
S Block elements
Groups 1 and 2, the alkali metals and the alkaline earth metals. Characterized by full or partially filled S orbitals.
P block elements
Groups 13-18 with valence electrons in the P orbital. Characterized by full or partially filled P orbitals.
D block elements
Contains the transition metals; is the largest of the blocks. Characterized by full or partially filled D orbitals.
F block elements
Contains the inner transition metals. Characterized by full or partially filled F orbitals.
Atomic Radius
Half the distance between adjacent nuclei of a crystal of an element, or half the distance between nuclei of identical atoms that are chemically bonded to each other.
The atomic radius increases as you go _____ and _____
Down and left.
Explain the atomic radius period trend.
As you go across a period, there are more protons, but they are all on the same energy level. Therefore, since the atomic charge is greater, the atomic radii get smaller. Valence electrons, because the principal energy level is the same, do not get increased shielding from the positive charge.
Explain the atomic radius group trend.
The atomic radii increase as you go down a group because as you go down a group, there are more energy levels. Therefore, the atomic radius gets bigger. The nuclear charge pull is overpowered because there is increased shielding from the positive charge.
Ion
An atom or bonded group of atoms that has a positive or negative charge
Ionic radius period trend
As you go across a period, the representative elements on the left side form increasingly small ions. Then, beginning in group 5A, the size of much larger negative ions gradually decreases.
Explain the Ionic radius period trend
Atoms on the left side of the periodic table lose electrons, so they become smaller. Atoms on the right side gain electrons so they become bigger.
Ionic radius group trend
As you go down a group, the atoms get bigger, so the ionic radii get bigger as well.
Ionization energy
The energy required to move an electron from a gaseous atom.
Ionization energy trends
As you go across a period, it gets bigger. However, there are some exceptions. An atom would rather have sets of full orbitals, so occasionally, the period trend will be broken. As you go down a group, the IE gets smaller because the electrons are further away from the nucleus.
Octet rule
Atoms tend to gain, lose, or share electrons in order to acquire a full set of eight valence electrons.
Electronegativity
The ability of an element to attract electrons in a chemical bond
Electronegativity trend
As you go from left to right, there is increasing electronegativity. As you go from top to bottom there is decreasing electronegativity. F is the most electronegative element.
Diagonal relationships
Some elements in period 2 do not behave as predicted by their locations on the table. Often, these elements have more in common with the period 3 element in the next group.
