The Periodic Table and Periodic Law Study Guide
S-BLOCK Periodic Table Group(s): ____(a)____ Orbital: ____(b)____ P-BLOCK Periodic Table Group(s): ____(c)____ Orbital: p D-BLOCK Periodic Table Group(s): 3 through 12 Orbital: ____(d)____ F-BLOCK Periodic Table Group(s): ____(e)____ Orbital: ____(f)____
(a): 1 and 2 (and 18 at 1st level) (b): s (c): 13 through 18 (d): d (e): 3 (f): f
All elements in group 1 have ______(a)______. All elements in group 2 have ________(b)_______. Group 13 elements have _______(c)________, group 14 elements have _______(d)_______, and so on. Helium, in group 18, is an _____(e)_____.
(a): 1 valence electron (b): 2 valence electrons (c): 3 valence electrons (d): 4 valence electrons (e): exception
Group: Strontium has a valence configuration of ____(a)____. All group ____(b)____ elements have the ____(c)____ configuration. Period: The ____(d)____ in 5s² indicates that strontium is in ____(e)____. Block: The ____(f)____ indicates that strontium's valence electrons ____(g)____. Therefore, strontium is in the ____(h)____.
(a): 2+ (b): 2 (c): 2+ (d): 5 (e): period 5 (f): s² (g): are in the s-orbital (h): s-block
The periodic table has ____(a)____ rows called periods. The table has ____(b)____ columns called ____(c)____ or families.
(a): 7 (b): 18 (c): groups
In 1869, _______________(a)___________. He left blank spaces ________________(b)___________.
(a): Dmitri Mendeleev published first periodic table (b): for undiscovered elements
In 1913, _______________(a)______________. He arranged elements by _______(b)_______.
(a): Henry Moseley discovered that every element has a unique proton count and corrected Mendeleev's periodic table (b): atomic number
In 1864, ___________(a)___________ and saw the properties of elements ______(b)_______.
(a): John Newlands created the Law of Octaves (b): repeat every 8th element
Ionization energies generally ____(a)____ as you move left-to-right across a ____(b)____. Increased nuclear charge leads to an ____(c)____ on valence electrons. Ionization energy generally ____(d)____ when you move down a ____(e)____. Less energy is required to remove ____(f)____ because they are ____(g)____ from the nucleus. The octet rule states that atoms tend to gain, lose, or share ____(h)____ in order to acquire a full set of ____(i)____. First period elements are the ____(j)____.
(a): increase (b): group (c): increased pull (d): decreases (e): group (f): electrons (g): farther (h): electrons (i): octets (j): exception
When an atom ____(a)____ electrons, its ion charge becomes positive, and its (the atom's) size ____(b)____. When an ____(c)____ gains ____(d)____, its ion charge becomes ____(e)____, and its (the atom's) size increases.
(a): loses (b): decreases (c): atom (d): electrons (e): negative
Analyze any trends that you observe on the periodic table and how the trends relate to atomic mass.
Atomic mass generally increases from left-to-right and top-to-bottom, although not all the time. As the atomic number increases, the mass increases as well (for the most part).
Infer how many electrons carbon is likely to lose.
Carbon would likely lose four electrons.
Define groups and periods
Groups are columns of elements while periods are rows of elements.
Xenon, a nonreactive gas used in strobe lights is a poor conductor of heat and electricity. Would you expect xenon to be a metal, a nonmetal, or metalloid? Where would you expect it to be on the periodic table? Explain.
I would expect it to be a nonmetal in the noble gases group because nonmetals are usually poor conductors of heat and electricity, and noble gases are nonmetals that are known for being highly unreactive
Determine the differences in electronegativity, ionic radius, atomic radius, and first ionization energy for oxygen and beryllium.
In comparison to beryllium, oxygen has higher levels of electronegativity, smaller ionic radius, smaller atomic radius, and higher first ionization energy.
Compare and contrast the ways in which Mendeleev and Moseley organized the elements.
Mendeleev organized by atomic mass while Moseley organized by atomic number. Both categorized by group and period. Both left spaces for undiscovered elements.
Describe the general characteristics of metals, nonmetals, and metalloids.
Metals are good conductors of heat and electricity, are solid at room temperature, and are ductile and malleable. Nonmetals are gases or dull, brittle solids that are poor conductors of heat and electricity. Metalloids retain properties from both metals and non-metals.
Explain why it takes more energy to remove the second electron from a lithium atom than it does to remove the fourth electron from a carbon atom.
The closer the electron is to the nucleus, the harder it is pulled to it. The opposite is true when it is farther away.
Identify one reason why the relative size of an atom becomes smaller due to the loss of electrons.
The ratio of electrons to protons pulling on them decreases. When that happens, the remaining electrons are pulled into the nucleus even more so, thus reducing the size of the atom.
Identify the information that is given on a typical box from the periodic table.
They are the name of the element, its symbol, its atomic mass, and its atomic number.
Period
a horizontal row of elements in the modern periodic table
Inner transition metal
a type of group B element that is contained in the f-block of the periodic table and is characterized by a filled outermost orbital, and filled or partially filled 4f and 5f orbitals
Group
a vertical column of elements in the periodic table arranged in order of increasing atomic number; also called a family
Indicate whether fluorine or bromine has a larger value for each of the following properties. a. electronegativity b. ionic radius c. atomic radius d. ionization energy
a. = fluorine b. = bromine c. = bromine d. = fluorine
Locate each of the following groups of elements on the periodic table. a. alkali metals b. alkaline earth metals c. inner transition metals d. nonmetals e. representative elements f. transition elements g. halogens h. transition metals i. noble gases
a. = group 1 (excluding Hydrogen) b. = group 2 c. = period 6-7 group 3 d. = period 1 group 18 period 2 group 14-18 period 3 group 15-18 period 4 group 16-18 period 5 group 17-18 period 6 group 18 e. = period 1-7 group 1-2 and 13-18 f. = period 4-7 group 3-12 (including inner transition metals) g. = group 7 h. = period 4-5 group 3-12 period 6-7 group 4-12 i. = group 18
Determine in which block of the periodic table the elements having the following valence electron configuration are located. a. s²p⁴ b. s¹ c. s²d¹ d. s²p¹
a. = p-block b. = s-block c. = d-block d. = p-block
Identify each of the following as a representative element or a transition element. a. lithium (Li) b. platinum (Pt) c. promethium (Pm) d. carbon (C)
a. = representative element b. = transition element c. = transition element d. = representative element
For each of the following elements, list two other elements with similar chemical properties. a. iodine (I) b. barium (Ba) c. iron (Fe)
a. = similar to fluorine (F) and chlorine (Cl) b. = similar to strontium (Sr) and calcium (Ca) c. = similar to ruthenium (Ru) and osmium (Os)
Ion
an atom or bonded group of atoms with a positive or negative charge
Transition metal
an element in groups 3-12 that is contained in the d-block of the periodic table and, with some exceptions, is characterized by a filled outermost s orbital of energy level n, and filled or partially filled d orbitals of energy level n-1
Metal
an element that is solid at room temperature, a good conductor of heat and electricity, and generally is shiny; most metals are ductile and malleable
Noble gas
an extremely unreactive group 18 element
Representative elements
elements from groups 1, 2, and 13-18 in the modern periodic table, possessing a wide range of chemical and physical properties
Transition elements
elements in groups 3-12 of the modern periodic table and are further divided into transition metals and inner transition metals
Nonmetals
elements that are generally gases or dull, brittle solids that are poor conductors of heat and electricity
Alkali metals
group 1 elements, except for hydrogen, they are reactive and usually exist as compounds with other elements
Alkaline earth metals
group 2 elements in the modern periodic table and are highly reactive
Electronegativity
indicates the relative ability of an element's atoms to attract electrons in a chemical bond
Octet rule
states that atoms lose, gain, or share electrons in order to acquire the stable electron configuration of a noble gas
Periodic law
states that when the elements are arranged by increasing atomic number, there is a periodic repetition of their properties
Valence electrons
the electrons in an atom's outermost orbitals; determine the chemical properties of an element
Ionization energy
the energy required to move an electron from a gaseous atom; generally increases in moving from left-to-right across a period and decreases in moving down a group
Atomic number
the number of protons in an atom
