chemistry chapter 10
atomic number
as a result of Henry Moseley's work, the modern periodic table is arranged in order of increasing
protons
atomic number of an element indicates the number of _ in the nucleus
electron affinity
attraction an atom has for an electron is called
family
because elements in a group may have similar characteristics, another name for a group is a(n) _
sheildin effect
causes ionization energy to decrease going down a column of the periodic table
T
each time a new principle energy is started, a new (row) in the periodic table begins
T
electron configuration of hydrogen and helium are (not similar), so they are in separate columns
diatomic elements
electrons that form covalent bonds with like atoms and are never found alone in nature are called
metalloid
element called _ has both metallic and nonmetallic properties
metal
element that has low electron affinity is classified as a(n) _
nonmetal
element with high ionization energy is classified as _
atomic mass
elements in Mendeleev's table were arranged by increasing
F; transition elements
elements in columns 3 through 12 are called (noble gases)
lanthanoid series
elements lanthanum through ytterbium, are contained in the set of elements called the _
first
energy necessary to remove completely the most loosely held electron from an atom is called the _ ionization energy
metal
hard, shiny, conducts heat and electricity well
F; series/period
in the periodic table, a horizontal row is called a (family)
period or series
in the periodic table, all elements in a horizontal row are referred to as a(n) _ or _
group or family
in the periodic table, all elements in the same vertical column form _ or _
transition elements
in the periodic table, elements in column 3 through 12 are called
Mendeleev
known as the "Father of the Periodic Table"
-3
oxidation number: 1s^2 2s^2 2p^3
-2
oxidation number: 1s^2 2s^2 2p^6
+1
oxidation number: 1s^2 2s^2 2p^6 3s^1
+2
oxidation number: 1s^2 2s^2 2p^6 3s^2
actinoid series
set of elemetns called _ contain elements actinium through nobelium
BrINClHOF
seven diatomic elements are
periodic table
shows placement of elements with similar electron configuration in columns in order of their increasing principle quantum numbers
ionic radius
size of an atom expressed interms of
I
smaller: Br or I
Ba
smaller: Cs or Ba
F
smaller: F or F-
K+
smaller: K or K+
Na
smaller: Na or Li
Ar
smaller: Ne or Ar
octet rule
states that an atom with eight electrons in its outer level is unreactive
periodic law
states that the properties of the elements are a periodic function of their atomic numbers
atomic number
the _ of an element is determined experimentally by x-ray diffraction of a crystal of the element
electron affinity
the attraction of an atom for an additional electron is called
ionization energy
the energy needed to remove an electron from an atom
first ionization energy
the energy needed to remove the most loosely held electron in an atom
T
the lanthanoid series contains the elements lanthium through (ytterbium)
7d
the pattern of placing electrons in energy sublevels for elements in the actenoid series
atom radius
the size of the atom is measured in terms of
they have full outer shells
what do neon and helium have in common
nonmetal
when forming compounds a(n)_ frequently gains electrons and can also share its outer electron with other atoms
smaller
when metallic atoms lose electrons, do they form ions that are smaller or larger than the original atoms?
larger
when nonmetallic atoms gain electrons, do they for ions that are smaller or larger than the original atoms?
noble gas configuration
when they have a(n) __, ions have a stable, filled outer level
increase
within a family, does the size of an atom generally increase or decrease with increasing atomic number?
decrease
within a period, does the size of an atom generally increase or decrease with increasing atomic number?