- show the arrangement of electrons within each energy level

Lecture 2 Flashcards by jai aji jjj leechai

Charge of electrons

1.6 × 10-19 coulombs

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Charge of protons

+ 1.6 × 10-19 coulombs (same with electrons but different sign)

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charge of neutron

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mass of electrons

9.11 × 10-31 kg

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mass of protons

1.67 × 10-27 kg

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mass of neutrons

1.67 × 10-27 kg

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gives chemical identification of the element

atomic number

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defines the isotope number

number of neutrons

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property of the principal orbit and its symbol

orbital size and energy level
symbol: n
positive numbers

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property of the secondary (angular momentum) orbit and its symbol

orbital shape (sublevels/subshells)
symbol: l 
0 to (n-1)

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1 mole = ______ atoms (or molecules

6.023 × 10^23

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All have the outer configuration s1

group 1 elements

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Electron configuration

associates the energy level with the number of

electrons in each level

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Orbital diagrams

show the arrangement of electrons within each

energy level

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– energy levels or energy shell

Period number

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have same sub shell or sub level

Group number –

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Distribution and arrangement of electrons in an atomic

orbital from lowest to highest energy

. – Aufbau Principle

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– Two electrons may occupy an orbital; with opposite spin

Paulis Exclusion Principle

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– distribution of the electron: occupy first each

Hund’s Rule

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t or f: Atoms of elements in a period have the same
distribution of electrons in the outermost principal
energy lev

false, group

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groups 13-18 fills what sublevel?

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p sublevel

occupies the d sublevels

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transition metals

occupies the f sublevels

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lanthanides and actinides groups

Elements in the same
column (Elemental Group)
share similar?

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properties.

Group number indicates the | number of?

electrons | available for bonding.

In a periodic table, Atomic size ______ in a group

increases

In a periodic table, ionization energy ______ in a group

decreases

In a periodic table, electron affinity ______ in a group

decreases

In a periodic table, electronegativity ______ in a group

decreases

In a periodic table, metallic ______ in a group

increases

In a periodic table, nonmetallic ______ in a group

decreases

In a periodic table, atomic size ______ in a period

decreases

In a periodic table, ionization energy ______ in a period

increases

In a periodic table, electron affinity ______ in a period

increase

In a periodic table, electronegativity ______ in a period

increase

In a periodic table, metallic ______ in a period

decrease

In a periodic table, nonmetallic ______ in a period

increase

a measure of how willing atoms are to | accept electrons

electronegativity

energy unit convenient for description of | atomic bonding.

electron volt (eV)

1 eV = ______ J

1.6 x 10-19 J

strong (100-1000 KJ/mol or 1-10 eV/atom) - results from the electron sharing or transfer

primary bonding

strong (100-1000 KJ/mol or 1-10 eV/atom) - results from the electron sharing or transfer

ionic bonding, primary bonding

electrons are shared between the molecules, to saturate the valency

covalent bonding, primary bonding

the atoms are ionized, loosing some electrons from the valence band. Those electrons form a electron sea, which binds the charged nuclei in place

metallic bonding, primary bonding

no e- transferred or shared - interaction of atomic/molecular dipoles - weak (< 100 KJ/mol or < 1 eV/atom

Secondary Bonding

Fluctuating Induced Dipole

secondary bonding, inert gases (H2, Cl2)

Permanent dipole bonds

(polar molecules - H2O, HCl...)

Polar molecule-induced dipole bonds

(a polar molecule induces a | dipole in a nearby nonpolar atom/molecule)

semiconductors bonding

covalent (most), ionic (small)

metals bonding

metallic bonding

ceramics bonding

covalent (small, ionic (most)

polymers bonding

covalent

Lecture 2 Flashcards

(52 cards)