This document provides information about the transition element titanium. It discusses the discovery of titanium, its sources in nature, physical and chemical properties, reactions, and common uses. Key points include that titanium is the ninth most abundant element in the Earth's crust, is commonly found in minerals like rutile and ilmenite, and reacts with oxygen, halogens, and acids. It is used to make aircraft and ships due to its high strength and corrosion resistance.

1. Transition Element
IV B GROUP
• Masita Saragih (06101010011)
• Narti Agustinah (06101010023)
• Paramita Dewi (06101010025)
• Murtiarni Putri (06101010026)
• Nora P Simamora (06101010035)

2. titanium
• From the Latin titans, the first
sons of the Earth, Greek
mythology.
• Discovered by Gregor in 1791;
named by Klaproth in 1795.
Impure titanium was prepared by
Nilson and Pettersson in 1887;
however, the pure metal (99.9%)

3. Sources
• Titanium is present in meteorites
and the sun. Rocks obtained during
the Apollo 17 lunar mission showed
presence of 12.1% TiO2; rocks
obtained during earlier Apollo
missions show lower percentages.
• Titanium oxide bands are prominent
in the spectra of M-type stars. The
element is the ninth most abundant
in the crust of the earth. Titanium is

4. • It occurs in the minerals rutile,
ilmenite, and sphene, and is
present in titanates and in many
iron ores. Titanium is present in ash
of coal, in plants, and in human
body.
• The metal was a laboratory
curiosity until Kroll, in 1946, showed
that titanium could be produced
commercially by reducing titanium
tetrachloride with magnesium. This
method is still largely used for

5. Atomic number 22
Atomic symbol Ti
Atomic weight 47.88
Electron configuration [Ar]4s23d2
Atomic radius 187 pm
Elektronegativity 1.54
Density 4.54 g/cm3
Melting point 1668 C
Boiling Point 3287 C
Oxidation States 4,3,2
Ionization potential 4.82 V
Crystal stucture Hexagonal

6. Reaction Of Titanium
• Reaction with water
Ti(s) + 2H2O(g) → TiO2(s) + 2H2(g)
• Reaction with air
Ti(s) + O2(g) → TiO2(s)
2Ti(s) + N2(g) →TiN(s)
• Reaction with Halogen
Ti(s) + 2F2(s) → TiF4(s)
Ti(s) + 2Cl2(g) → TiCl4(s)
Ti(s) + 2Br2(l) → TiBr4(s)
Ti(s) + 2I2(s) → TiI4(s)

7. • Reaction with acid
Titanium does not react with mineral
acid in normal temperature but react
with hot hidrofluorik acid become
complex anion (TiF6)3-
2Ti(s) + 2HF (aq) → 2(TiF6)3-(aq) + 3
H2(g) + 6 H+(aq)
• Reactio with base
Titanium does not react with alkali in
normal temperature, but in hot

8. Uses
• Manufacture of aircraft and warship
• Titanium has potential use in desalination
plants for converting sea water into fresh
water
• Used to provide cathodic protection from
corrosion by salt water
• Titanium dioxide is extensively used for both
house paint and artist's paint

9. ZIRCONIUM
• From the Persian zargun, gold like. Zircon, the
primary gemstone of zirconium, is also known
as jargon, hyacinth, jacinth, or ligure
• The metal is found by M.H.Kalaproth in 1788
from of mineral zircon
• Zyrconium metal is grayish white,
crystalin,soft,malleabel and can be stretched
when in pure condition and resistant whith air
and fire.

10. Sources
• Zirconium is produced from the
mineral zircon (ZrSiO4).
• It is found in abundance in S-type
stars, and has been identified in
the sun and meteorites.
• Analysis of lunar rock samples
obtained during the various Apollo
missions to the moon show a

11. Atomic number 40
Atomic symbol Zr
Atomic weight 91.22
Electron configuration [Kr]5s24d2
Atomic radius 186 pm
Elektronegativitas 1.33
Kerapatan 6.506 g/cm3
Melting point 1855 C
Boiling Point 4409 C
Oxidation States 4
Ionization potential 6.84 V
Crystal stucture Hexagonal

12. Reaction of Zirconium
• Reaction with water
Zirconium does not react with water in
unnormal condition .
• Reaction with air
Zr (s) + O2 (g) → ZrO2 (s)
• Reaction with halogen
Zr (s) + 2F2 (g) → ZrF4 (s)
Zr (s) + 2Cl2 (g) → ZrCl4 (s)
Zr (s) +2Br2 (g) → ZrBr4 (s)
Zr (s) + 2I2 (g) → ZrI4 (s)

13. Uses
• Zirconium is used as a getter in vacuum tubes
• used extensively by the chemical industry
where corrosive agents are employed
• as an alloying agent in steel, in surgical
appliances, photoflash bulbs, explosive
primers, rayon spinnerets, lamp filaments
• With niobium, zirconium is superconductive at
low temperatures and is used to make
superconductive magnets

14. Hafnium
• From Hafinia, the Latin name for
Copenhagen. Many years before its
discovery in 1932 Hafnium was thought
to be present in various minerals and
concentrations.
• Metallic hafnium was first prepared by
van Arkel and deBoer by passing the
vapor of the tetraiodide over a
heated tungsten filament
• Zirconium and hafnium are two of the
most difficult to separate. Although their

15. Atomic number 72
Atomic symbol Hf
Atomic weight 178.49
Electron configuration [Xe]6s24f145d2
Atomic radius 212 pm
Elektronegativitas 1.30
Density 13,31 g/cm3
Melting point 2233 C
Boiling Point 4602 C
Oxidation States 4
Ionization potential 6.65
Crystal stucture Hexagonal

16. Reaction Of Hafnium
• Reaction with water
Hafnium does not react with water at
unnormal.
• Reaction with air
Hf (s) + O2 (g) → HfO2 (s)
• Reaction with Halogen
Hf (s) +2F2 (g) → HfF4 (s)

17. Uses
• Hafnium is used for reactor
control rods
• Hafnium is used in gas-filled and
incandescent lamps, and is an
efficient getter for
scavenging oxygen and nitrogen
• used as a gas filled in plasma
cutting