group 14 Flashcards
(32 cards)
What elements belong to Group 14?
Carbon, silicon, germanium, tin, lead, and flerovium.
What is the 17th most abundant element by mass in Earth’s crust?
Carbon.
In what forms is carbon found in nature?
Free state: coal, graphite, diamond. Combined state: metal carbonates, hydrocarbons, CO2 (0.03%) in air.
Why is carbon considered the most versatile element?
It combines with elements like H2, O2, Cl, and S to form diverse materials, from living tissues to plastics and drugs.
What is the branch of chemistry that focuses on carbon-containing compounds?
Organic chemistry.
What are the stable isotopes of carbon?
¹²C and ¹³C.
What is the third isotope of carbon, and what is its significance?
¹⁴C is a radioactive isotope with a half-life of 5770 years, used in radiocarbon dating.
What is the second most abundant element in Earth’s crust?
Silicon (27.7% by mass).
In what forms is silicon naturally found?
Silica and silicates.
What materials commonly use silicon?
Ceramics, glass, and cement.
In what amount does germanium exist in nature?
Only in trace amounts.
What are the main ores of tin and lead?
Tin: cassiterite (SnO₂), Lead: galena (PbS).
What is flerovium, and how is it obtained?
A synthetically prepared radioactive element.
What are ultrapure forms of germanium and silicon used for?
Making transistors and semiconductor devices.
general electronic configuration
ns2 np2
Atomic radius
C< Si< Ge< Sn< Pb
How does the covalent radius change in Group 14 elements?
Increases considerably from C to Si, then a small increase from Si to Pb due to filled d and f orbitals.
Ionisation energy
C >Si> Ge> Pb>Sn
How does the first ionization enthalpy of Group 14 compare to Group 13?
Higher in Group 14 due to inner core electron influence.
What is the general trend of ionization enthalpy in Group 14?
Decreases down the group due to increasing atomic size and shielding effect. exception on pb and Sn
Why is there a slight increase in ionization enthalpy from Sn to Pb?
Due to poor shielding effect of d and f orbitals despite size increase.
Electronegativity of group 14
C>Pb>SI=Ge=Sn
How does electronegativity in Group 14 compare to Group 13?
Group 14 elements are slightly more electronegative than Group 13.
How does electronegativity change from Si to Pb?
Electronegativity values remain almost the same from Si to Pb.
