Chapter 14 - Periodic Patterns in the Main-Group Elements

Atomic size

________ typically reduces when nuclear charge increases and electrons are added to orbitals of the same energy level (same n value), but initial ionization energy and electronegativity often rise (see bar graphs)

covalent hydrides

Many ___________ are formed when hydrogen interacts with nonmetals, including CH4, PH3, H2S, and HCl.

H−

In water, ________ is a strong base that pulls H+ from surrounding H2O molecules to form H2 and OH−:

Metals

________ reduce strength, whereas nonmetals improve strength.

Hydrogen

like the elements of Group 7A (17), exists as diatomic molecules and fills its outer level either via electron sharing or by acquiring one electron from metal to create a 1 ion (hydride, H)

noble gas

Except for the inert ________, reactivity is strongest at the left and right ends of the period because members of Groups 1A (1) and 7A (17) are just one electron away from achieving a filled outer level.

covalent hydrides

The conditions for producing ________ are determined by the reactivity of the other nonmetal.

monatomic halide ions

While ________ (X) are abundant and stable, H is uncommon and reactive.

hydride ion

The ________ is also a powerful reducing agent; for example, it reduces Ti (IV) to the free metal:

hydrogen atom

A(n) ________ is made up of a single positive- charged nucleus surrounded by a single electron.

alkali metals

Unlike ________, however, hydrogen shares its single valence electron with nonmetals rather than transferring it to them.

individual molecules

The bonding between an element's atoms evolve from metallic to covalent in networks, covalent in ________, and none (noble gases exist as separate atoms)

Hydrogen

________ may be the most significant element of all because of its simple structure.