The Periodic Table

Front 1

What is periodic about the periodic table of elements?

Back 1

As atomic number increases, the physical and chemical properties of elements repeats at regular intervals.

Front 2

Why is Mendeleev known as "The father of the Periodic Table"?

Back 2

Mendeleev was the first scientist to organize the elements in a table

Front 3

explain how mendeleev was able to predict the properties and atomic masses of several undiscovered elements.

Back 3

empty spaces in mendeleev's table corresponded to undiscovered elements

Front 4

how was moseley's organization of the elements different from mendeleev's

Back 4

mendeleev organized the elements by atomic mass. Moseley organized the elements by atomic number

Front 5

for each of the following types of elements, tell their location on the periodic table, and the physical and chemical properties they have in common:
a. noble gases
b. halogens
c. lanthanides
d. alkaline earth metals
e. actinides
f. alkali metals
g. transitiion metals
h. metalloids

Back 5

a. noble gases: group 18, colorless gases, very low reactivity
b. halogens: group 17, nonmetals/highly reactive
c. lanthanides: #57 to #70, metals/radioactive/rare
d. alkaline earth metals: group 2, metallic, reactive
e. actinides: #89-102, radioactive, most artificial
f. alkali metals: group 1, shiny, soft, highly reactive
g. transition metals: d-block, shiny-low reactivity
h. metalloids: stairstep between metals and nonmetals, partially conductive of heat and electricity

Front 6

Explain why elements within the same group tend to have similar chemical properties

Back 6

elements in the same group have similar outer electron configurations and the same number of valence electrons

Front 7

what happens to atomic radii as you go across the table, and why

what happens to atomic radii as you go down the table and why

Back 7

atomic radius decreases across the periodic table because additional protons in nuclus attract the electrons more

atomic radius increases down a group because the outer electrons are in higher energy levels and are less attracted to the nucleus.

Front 8

what is ionization energy?

Back 8

ionization energy is the amount of energy that is required to remove one electron from an atom

Front 9

what happens to ionization energy as you go across the periodic table and why

what hapens to ionization energy as you go down the table, and why

Back 9

ionization energy increases across the periodic table because there are more protons in the nucleus that attract the electrons. When the electrons are attracted, it is more difficult for them to be taken away.

Down the table, ionization energy decreases because there are more energy levels and the valence electrons are further away from the attraction of the nucleus, making less energy required to remove them.

Front 10

explain the difference between ionization energy and electron affinity.

Back 10

ionization energy is the amount of energy that is added when an electron is taken away from an atom. Electron affinity is the amount of energy that is released when one electron is added.

Front 11

what is electronegativity?

Back 11

electronegativity is the tendency of an atom to attract electrons when in a compound.

Front 12

what happens to electronegativityas you go across the periodic table, and why?

what happens to electronegativity as you go down the periodic table, and why?

Back 12

electronegativity increases across periodic table because valence electrons are more attracted to the more positive nucleus.

electronegativity decreases down a group because valence electrons are further from the nucleus and less attracted to it.

Front 13

explain the octet rule.

Back 13

the octet rule states that an atom is most stable when its valence level is completely filled with eight electrons.

Front 14

what is an ion

Back 14

an ion is an atom or molecule with a net positive or negative charge.

Front 15

when electrons are removed from an atom... does the atom become positively or negatively charged?
does the atom become bigger or smaller?

Back 15

the atom becomes positively charged smaller... the atom becomes smaller because the electrons go away.

Front 16

when electrons are added to an atom, does the atom become positively or negatively charged?

does the atom become bigger or smaller?

Back 16

the atom becomes negatively charged and the atom becomes bigger

Front 17

which groups of elements would be more likely to make negative ions? group 2 or 17? explain.

Back 17

group 17 would because it would gain electrons which is equivalent to gaining negative charges.

Front 18

distinguish between cations and anions

Back 18

cations are positive because they are missing electrons and anions are negative because they have extra electrons.