Pharm Chem 11 - Group of Elements and their General Properties

*old IUPAC name* - *new IUPAC name* recommend using ma'am's mnemonics. for lists, type the word, comma, space, then the next word. Recommend using text answer because there are different definitions with the same term, causing it to possibly duplicate on some items in mpc.

group 1 a - group 1

alkali metals

group 1 b - group 11

coinage metals

group 2 a - group 2

alkaline earth metals

group 2 b - group 12

volatile metals / zinc group

group 3 a - group 13

icosagens / boron family

group 3 b - group 3

scandium subgroup

group 4 a - group 14

crystallogens / carbon family

group 4 b - group 4

titanium subgroup

group 5 a - group 15

pnictogens / nitrogen family

group 5 b - group 5

vanadium subgroup

group 6 a - group 16

chalcogens / oxygen family

group 6 b - group 6

chromium subgroup

group 7 a - group 17

halogen family

group 7 b - group 7

manganese subgroup

group 8 a - group 18

inert gases

group 8 b & group 9 - group 8 & 9

iron triad

list alkali metals

hydrogen, lithium, sodium, potassium, rubidium, cesium, francium

list coinage metals

copper, silver, gold

list alkaline earth metals

beryllium, magnesium, calcium, strontium, barium, radium

list volatile metals

zinc, cadmium, mercury

list icosagens / boron family

boron, aluminum, gallium, indium, thallium

list scandium subgroup

scandium, yttrium, lanthanide series, actinide series

list crystallogens / carbon family

carbon, silicon, germanium, tin, lead

list titanium subgroup

titanium, zirconium, hafnium

list pnictogens / nitrogen family

nitrogen, phosphorus, arsenic, antimony, bismuth

list vanadium subgroup

vanadium, niobium, tantalum

list chalcogens / oxygen family

oxygen, sulfur, selenium, tellurium, polonium

list chromium subgroup

chromium, molybdenum, tungsten, uranium, seaborgium

list halogen family

fluorine, chlorine, bromine, iodine, astatine

list manganese subgroup

manganese, technetium, rhenium

list inert / noble gases

helium, neon, argon, krypton, xenon, radon

list iron triad

iron, cobalt, nickel

list platinum group metals

ruthenium, palladium, rhodium, iridium, osmium, platinum

list light platinum group metals

ruthenium, palladium, rhodium

list heavy platinum group metals

iridium, osmium, platinum

alkali metals

very good reducing agents, they can easily loose an electron, low I.P.

alkali metals

atoms are large with only 1+ valence electron at the S orbitals

alkali metals

very active metals with reactivity increasing with atomic weight

alkali metals

because of they have large atoms and very active, they are never found

nature in the free state

alkali metals

with +1 oxidation state thus they are usually in salts form ; univalent

hydrides

when alkali metals combine with hydrogen, they form

halides

when alkali metals combine with halogens, the form

oxides

when alkali metals combine with oxygen, they form

lithium

salts of alkali metals are the most water-soluble except for

alkali metals

are grey solids with shiny silvery surfaces when freshly cut.

alkali metals

They react rapidly with oxygen and water vapour in the air when exposed.

alkali metals

soft solids and can be easily cut

alkali metals

have low densities as compared to heavy metals such as iron and copper.

alakli metals

are good conductors of heat and electricity

alkali metals

have low melting and boiling points as compared to heavy metals such as copper and iron.

coinage metals

occur in nature in its free state

coinage metals

not chemically active or least reactive because they do not loose electron easily due to high I.P.

coinage metals

divalent ( display in multiple oxidation state)

coinage metals

valence electron is also 1+ at the d orbitals

coinage metals

insoluble in water

coinage metals

can react with oxygen to form oxides and hydroxides but are weak basic except for silver oxide

coinage metals

easily reduced but difficult to oxidize

coinage metals

all of the element under these group form complex anions and cations with ammonia ( NH3

coinage metals

most of these metals are used as ornamental and coinage purposes

coinage metals

FORMS COMPLEXES OR CHELATES

alkaline earth metals

strong reducing agents but not as strong as the elements under group 1

alkaline earth metals

these group loses 2 valence electrons forming 2+ ions

alkaline earth metals

chemical activity increases as atomic radius increases

alkaline earth metals

these metals combine directly with oxygen, halogens, N2 , S, H2 except for magnesium

alkaline (basic) solution

Mg reacts with steam liberating H2 gas and formation of

beryllium oxide amphoteric

oxides form are all basic except for

alkaline earth metals

group of metals where hydroxides form increases in strength as bases going down the group

alkaline earth metals

Ba and Be are the poisonous elements of this group

alkaline earth metals

Tend to be harder, more dense and have higher melting points than the alkali metals

less reactive

I₁ is low, but higher than the alkali metals, so it is

nitrides (M3N2)

What compounds do alkaline earth metals form when heated in nitrogen?

water

The alkaline earth metals react with ? to produce metal hydroxides and hydrogen gas.

beryllium and magnesium

for alkaline earth metals, they do not react readily with water due to low reactivity.

halogens

The alkaline earth metals react directly with ? to form metal halides.

Metal halides

Compounds formed when alkaline earth metals combine with halogens such as fluorine, chlorine, bromine, or iodine.

volatile metals

in compounds, these elements exist as divalent ions but Hg in addition has a unique property of having a monovalent ion as Hg2 2+

volatile metals

has an oxidation number of 2+

volatile metals

these metals react with halogens, oxygen, nitric acid and other common oxidizing agents

volatile metals

they form complex ions such as amines, cyano and halo-

volatile metals

they form adherent oxides or basic carbonate coating when exposed to air, which further prevent them from oxidation

volatile metals

the oxides and hydroxides of these metals are weak bases with base strength increasing going down the group

alloys

one of the principal uses of volatile metals is in the preparation of

volatile metals

electronically active contaminants that can cause device failure

volatile metals

in corrosive gas distribution systems, these metals are not removed by particle filters

volatile metals

widely used in electric and electronic applications

toxic

Cadmium and Mercury are both highly ?

icosagens / boron family

group of metals that has an oxidation number/state of 3+

icosagens / boron family

they readily oxidized when heated in air but they are stable at ordinary temperatures

Boron

other metals are poor or weak except for one which is the only nonmetal in the icosagens / boron family

Scandium subgroup

divalent, has oxidation number/state of 3+ or 2+

Scandium Subgroup

the elements of these group have physical properties that are typical metals

Scandium Subgroup

they are all quite reactive chemically and their oxides form are basic or alkalinic compounds

mixtures

all the lanthanide elements occur in ?, which are hard to separate due to similarity in chemical properties

crystallogens / carbon family

the elements may exhibit 2+ and 4+ oxidation states

germanium, tin, lead

elements in the carbon family which are rather active metals because they will be displaced by hydrogen gas from acids and combine with most nonmetals

crystallogens / carbon family

used as reducing agents in the preparation of many metals most are inert in room temperature

crystallogens / carbon family

can combine directly with oxygen and halogens as well as with other nonmetals

carbon

the only non-metal in the crystallogens / carbon family

silicon, germanium

metalloids in the carbon family

tin, lead, flerovium

metals in the carbon family