Unit 4: The Periodic Table

Question 1

electronegativity

Answer 1

tendency for the atoms of the elements to attract electrons during chem. reactions.

Question 2

the pauling scale relies on what two factors?

Answer 2

ionization energy and electron affinity

Question 3

ionization energy

Answer 3

the amount of energy needed to remove the highest energy electron from an element in its GASEOUS PHASE

Question 4

electron affinity

Answer 4

the change in energy when an electron is added.

Question 5

electroegativity trends in groups

Answer 5

electronegativity decreases down a group, because PEL’s are added going down a group which creates a greater atomic radius, decreasing the nuclear attraction that would increase electronegativity.

Question 6

shielding

Answer 6

the buffering of attraction between the positive nucleus and the outermost electron shell.

Question 7

electronegativity with noble gases

Answer 7

they do not have electronegativity values because they were historically thought to not bond, and even though they sometimes do, no values were assigned anyways.

Question 8

electronegativity trends down a period

Answer 8

from left to right, electronegativity increases, since the valence electrons become more full, making it easier to gain electrons to fill up the shell, and atomic radius decreases as the nuclear attraction increases.

Question 9

What is the element with the lowest electronegativity?

Answer 9

cesium, with only 1 valence electron and the largest atomic radius

Question 10

what is the element with the highest electronegativity

Answer 10

fluorine, small atomic radius and high # of valence electrons.

Question 11

cation

Answer 11

atom that loses electrons, a positively charged ion.

Question 12

what kind of elements form cations?

Answer 12

metals since they have leses valence electrons, easier to lose than gain to create a full octet/duet.

Question 13

Is a cations radius smaller or larger than the original atoms?

Answer 13

the radius is smaller, since the loss of the electron results in less shielding, making the attraction from the nucleus pull the electrons closer to the atom.

Question 14

anion

Answer 14

atom that has gained an electron, negatively charged

Question 15

what kinds of elements form anions?

Answer 15

nonmetallic anions, bc they have high ionization energies and readily gain electrons

Question 16

is the radius of an anion larger or smaller than that of the original atoms?

Answer 16

larger, because the addition of the electron makes the atom bulge due to electron-electron repulsion

Question 17

metalliods/semimetals

Answer 17

elements with properties between or in combination of those of nonmetals and metals.

Question 18

what are the six metalloids?

Answer 18

boron, silicon, germanium, arsenic, antimony, tellurium BATGAS

Question 19

what is the only metal that is liquid at STP?

Answer 19

mercury

Question 20

what is the only nonmetallic element that is liquid at STP?

Answer 20

bromine

Question 21

what are the only two elements on the periodic table that are liquid at STP?

Answer 21

bromine and mercury

Question 22

what is considered the most metallic element, chemically?

Answer 22

cesium (since francium is radioactive) because it has only one v-electron, has the largest radius due to many PELs, which causes shielding, and the lowest ionization energy.

Question 23

what group is the most reactive metallic elements?

Answer 23

alkali metals

Question 24

what is considered the most chemically nonmetallic element?

Answer 24

fluorine, since it has the smallest radius of all group 17 elements and only has 1 missing v-electron, allowing it to be the most attractive element.

Question 25

what are the most reactive non metallic elements?

Answer 25

group 17 halogens, who react with alkali metals, combining to form salts

Question 26

which group 18 elements have some chemical reactivity?

Answer 26

Xenon and Krypton have oxidation states other than 0, though noble gases all have full valence shells and are very stable as a result, and so usually will not bond.

Question 27

name the monatomic elements

Answer 27

group 18 noble gases

Question 28

name the diatomic elements

Answer 28

H O F Br I N Cl

Question 29

name the five elements that are gases at STP besides the noble gases

Answer 29

hydrogen, nitrogen, oxygen, fluorine, and chlorine. (the diatomic elements minus iodine and boron)

Question 30

after which number element are all elements considered naturally occurring radioactive isotopes?

Answer 30

#83

Question 31

allotropes

Answer 31

2 or more different molecular forms of the same element in the same physical state

Question 32

name the two allotropes of oxygen

Answer 32

ozone (O3) and oxygen gas (O2)

Question 33

name the three allotropes of carbon

Answer 33

diamond, graphite, and buckminsterfullerenes (C-60)

Question 34

atomic radius

Answer 34

half that distance between the nucleus of the 2 bonding atoms.

Question 35

measuring atomic radius

Answer 35

cannot be measured directly since atoms do not have defined boundaries, though there are many ways to estimate

Question 36

what are the two ways to estimate atomic radius?

Answer 36

- using X-ray diffraction if the element is a solid, crystalline structure, to estimate the distance between nuclei. - for diatomic elements it is only possible to estimate the distance between the nuclei of the two bonded atoms.

Question 37

atomic radius trends down a group

Answer 37

atomic radius increases as you go down a group, bc more PEL's are being added, increasing shielding as well.

Question 38

atomic radius trend across a period

Answer 38

generally decreases since the PEL remains the same while more and more v-electrons are added, increasing the NUCLEAR CHARGE while the shielding stays the same.

Question 39

in a single period, atomic radius and atomic number have an

Answer 39

INVERSE RELATIONSHIP

Question 40

when a substance is ionized it results in a...

Answer 40

1+ charge

Question 41

why are there jumps in ionization energy?

Answer 41

valence electrons are easy to take away, so they require low amounts of ionization energy to be stolen. Once they are all gone, it takes much more energy to take away a core electron, which accounts for the jump.

Question 42

what is the unit for ionization

Answer 42

kj/mol

Question 43

what element has the highest first ionization energy?

Answer 43

helium, because it has both a full electron shell and also the smallest atomic radius, which separates it from the rest of the noble gases, since a smaller radius = greater attraction = harder to steal the electron

Question 44

ionization group trends

Answer 44

as atomic # increases in group the ionization energy decreases, since the PELs increase, increasing shielding, which makes it easier to steal the electron.

Question 45

ionization trends across a period

Answer 45

first ionization energy increase across a period, since the nuclear charge increases, strengthening the hold on the electrons.

Question 46

which subatomic particle effects chemical and physical properties the most?

Answer 46

the electron

Question 47

the arrangement of the periodic table is related to

Answer 47

electron configuration

Question 48

what are the four categories electrons can be classified into based on electron configuration?

Answer 48

noble gases, rep. elements, transition metals, and inner transition metals.

Question 49

electron confg: noble gases

Answer 49

they have a full outer shell and are inert gases bc they do not bond, belonging to block p except for Helium, which is in the s block.

Question 50

electron config: representative elements

Answer 50

- elements with outermost p and s sublevels only partially filled - group number tells you the number of valence electrons - the representative element group names are the alkali metals, alkaline earth metals, and the halogens.

Question 51

electron config: transition metals

Answer 51

- group B elements - contains 3s elements - defined as the elements with an incomplete d orbital. - belongs to the d sublevel block but not all d-block elements are transition metals - electrons are added to the d sublevel rather than the outermost shell, disrupting the pattern - transition metals fill the PEL one less than the period number.

Question 52

electron config: inner transetals

Answer 52

- the lanthanides and actinide series, belonging to the F sublevel, where electrons are added to the f shell rather than the outermost shell and the PEL added to is 2 less than the period.

Question 53

electrno config: lanthanides

Answer 53

electrons are added to 4f

Question 54

electron config: actinides

Answer 54

electrons added to 5f

Question 55

dmitri mendeleev (1843-1907)

Answer 55

- mid 1800s arranged elements in vertical columns with increasing atomic mass, arranged by chem. and physical properties - blank spaces were from undiscovered elements - he could predict properties by comparing to the known elements.

Question 56

henry mosely (1887-1915)

Answer 56

- determined nuclear charge of the atom, aka the atomic # | - arranged the table according to atomic # like the modern periodic table.

Question 57

periodic law

Answer 57

when elements are arranged in order of increasing atomic number, there is a periodic pattern of chemical and physical properties

Question 58

what kinds of elements form compounds and solutions with COLOR

Answer 58

transition metals

Question 59

what kinds of elements have MULTIPLE oxidation states

Answer 59

transition metals

Question 60

name the four properties of metals

Answer 60

- malleable - ductile - luster - good conductors of both heat and electricity

Question 61

ductile

Answer 61

can be made into wire

Question 62

luster

Answer 62

ability to reflect light

Question 63

group 1 metals are so reactive that you will never find them _____ in nature, only in the form of _____

Answer 63

free, salts

Question 64

how do you extract the group 1 element from the compound

Answer 64

run electric current through it, Cl gas for example will evaporate and leave behind the group 1 element.