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