Chem-Ch6
period
horizontal rows
how does ionization energy change going across a period?
increases
Mendeleev
-"father of the periodic table" -arranged elements by increasing atomic mass and similar properties
does Fluorine or Iodine have a higher ionization energy level?
-Fluorine -because as you go down a group, the electrons are held more loosely by the nucleus -because less energy needed to remove an electron
which element is an exception to the Octet Rule and why?
-Helium -because Helium can only hold 2 electrons -it is stable with only 2 electrons
octet rule
-an atom's tendency to gain, lose, or share electrons in order to require a full set of valence electrons and to become stable. -s2p6 = 8 valence electrons, so 8 is a full orbital and what makes an atom stable -the d and f orbitals are not significant when counting the valence electrons, only add the s and p e-
what was the problem with Mendeleev's periodic table?
-arranged by increasing atomic mass which would put some elements in the wrong group
metalloids
-borders the staircase -except for Aluminum and Polonium -aka semi metals
chlorine is often used in swimming pools, what other element may be used in swimming pools to keep them clean?
-bromine -group 17, the halogens (similar properties in groups)
what are 3 special characteristics about Hydrogen?
-does not belong to any group -a nonmetal -placed above group 1 and sometimes above group 17
group 1 metals often react (blank) with water
-explosively -they become more and more reactive/explosive going down the group
list the metalloids
-boron -silicon -germanium -arsenic -antimony -tellurium -astatine -not aluminum or polonium
why does an atom become smaller after losing electrons?
electrons repel each other so removing an e- means the atom gets smaller
why does Fluorine have a smaller atomic radius than Carbon, Nitrogen, or Oxygen?
-greater number of protons in its nucleus, therefore, it has a stronger positive charge to pull in electrons -electrons are added to the same energy level
which would you expect to have more similarities, the elements in period 2 or the elements in group 2?
-group -because the same number of valence electrons -because elements have similar properties if they're in the same group
noble gases
-group 18 -full set of orbitals = already stable -s2p6 -does not include electronegativity rules -8 valence electrons
which group has the highest ionization energy? the lowest?
-group 18 the noble gases -group 1 the alkali metals
what are the two rows in the inner transition metals called?
-lanthanide series (period 6) -actinide series (period 7)
Newlands
-law of octaves -62 known elements so far -elements arranged by increasing atomic mass had similar properties between the 1st and 8th element
what did Mendeleev do with the blank spaces in his periodic table?
-made accurate predictions based on the other elements in each specific group
synthetic
-manufactured elements -transuranium -after element 92, uranium
protons remain protected in the (blank)
-nucleus -therefore, protons are not involved in ordinary chemical reactions
Mosley
-observed and identified the positive charge of the nucleus as the atomic number -arranged the elements by increasing atomic number -put elements such as Tellurium and Iodine in their correct groups
valence electrons
-outermost electrons of an atom -highest energy electrons -located farthest away from the nucleus -involved in ordinary chemical reactions
why did Mendeleev leave blank spaces in his periodic table?
-to ensure that elements with similar properties would be in the same group -believed that elements would be found/discovered and go into the spaces
Dobereiner
-triads -groups of 3 -based on similarities -30 known elements so far
ionic size
-when an element loses electrons, it becomes positive and smaller -when an element gains electrons, it becomes negative and bigger
periodic law
-when elements are arranged in increasing atomic number, their chemical and physical properties show a periodic pattern -every once in a while, the properties repeat
(blank) are grouped together according to similar (blank) and (blank) properties
elements, chemical, physical
inner transition metals
f block
elements on the right of the periodic table tend to (blank) electrons to become more stable.
gain
what would oxygen most likely do to become stable?
gain an e-
alkali metals
group 1
chalcogens
group 16
halogens
group 17
alkaline earth metals
group 2
how does electronegativity change going across a period?
higher electronegativity
electronegativity
an atom's ability to attract electrons
valence electrons are responsible for (blank)
an atom's chemical properties
the periodic table is arranged in order of increasing (blank)
atomic number
atomic mass
average mass of all isotopes of an element
how can you tell if an element is solid at room temperature?
black writing
how can you tell if an element is liquid at room temperature?
blue writing
transition metals
d block
how does ionization energy change going down a group?
decreases
atomic radius
distance from nucleus to outer electrons
why does an atom become bigger after gaining electrons?
electrons repel each other so adding even just one e- moves all the other e- away
what would happen to the charge of an oxygen atom that has become stable?
it would become negative
what would happen to the charge of a sodium atom that become stable?
it would become positive
how does atomic radius change going down a group?
larger
elements on the left of the periodic table tend to (blank) electrons to become more stable
lose
what would sodium most likely do to become stable?
lose an e-
how does electronegativity change going down a group?
lower electronegativity
atomic number
number of protons
metals
on the left side of the staircase
nonmetals
on the right side of the staircase
abbreviated electron configurations are important because they show the (blank) electrons in an atom
outer
how can you tell if an element is a gas at room temperature?
red writing
why do elements in a group share similar properties?
same number of valence electrons
how does atomic radius change going across a period?
smaller
metals are normally (blank) at room temperature
solid
ionization energy
the energy needed to remove an electron from an atom
group/family
vertical columns