ALL General Chemistry Flashcards (DAT)

Elements with unpaired electrons

paramagnetic

Elements with paired electrons

diamagnetic

Elements that are attracted to magnets

paramagnetic

Elements that are not attracted to magnets

diamagnetic

Percent composition formula

component molar mass / compound molecular mass

Formula that shows the most reduced ratio of atoms in a compound

empirical

Formula that shows the exact number of atoms of each element in a compound

molecular

Percent error formula

| experimental - actual | / actual

Percent yield

actual / theoretical

Atomic theory states that all matter is made up of indivisible ___

atoms

Atomic theory states that atoms of a specific element are identical in ___ and ___

mass and properties

Atomic theory states that compounds are formed by whole number ratios of ___ or more different atoms

two

Atomic theory states that a chemical reaction is a ___ of atoms

rearrangement

The sum of the number of protons and neutrons

mass number

The electron configuration rule which states that each orbital within a subshell must receive an electron before pairing

Hund’s rule

The electron configuration rule which states that all electrons within a singly occupied orbital must have the same spin, whether that’s all up or all down

Hund’s rule

The electron configuration rule which states that subshells get filled from lower to higher energy levels

Aufbau principle

In atomic notation, the upper left number represents the

mass number, protons + neutrons

In atomic notation, the bottom right number represents the

atomic number, protons

The common example of a physical change

phase change

Formula for the maximum number of electrons in each energy level

2n²

Molecular geometry of CO₂

linear

Bond angles of linear

180

Molecular geometry of BF₃

trigonal planar

Bond angles of trigonal planar

120

Molecular geometry of SO₂

bent

Bond angles of bent

<120

Molecular geometry of CH₄

tetrahedral

Bond angles of tetrahedral

109.5

Molecular geometry of NH₃

trigonal pyramidal

Bond angles of trigonal pyramidal

107.5

Molecular geometry of H₂O

bent

Molecular geometry of PCl₅

trigonal bipyramidal

Bond angles of trigonal bipyramidal

90, 120

Molecular geometry of SF₄

seesaw

Bond angles of seesaw

<90, <120

Molecular geometry of ClF₃

T-shaped

Bond angles of T-shaped

<90

Molecular geometry of XeF₂

linear

Molecular geometry of SF₆

octahedral

Bond angles of octahedral

90

Molecular geometry of ClF₅

square pyramidal

Bond angles of square pyramidal

<90

Molecular geometry of XeF₄

square planar

Bond angles of square planar

90

What elements are included in the half-filled electron configuration exceptions?

Cr, Mo

What elements are included in the filled electron configuration exceptions?

Cu, Ag, Au

In “2p⁶” the 2 stands for the

principal energy level, period the element is in

In “2p⁶” the p stands for the

subshell

In “2p⁶” the 6 stands for the

number of electrons

n stands for the ___ quantum number

principal

l stands for the ___ quantum number

angular momentum

m_l stands for the ___ quantum number

magnetic

m_s stands for the ___ quantum number

spin

Allowed values of n

positive integers (1, 2, 3)

Allowed values of l

0 to n-1

Allowed values of m_l

-l to +l

Allowed values of m_s

+1/2 or -1/2

Which quantum value conveys the orbital size and energy level

n

Which quantum value conveys the orbital shape

l

Which quantum value conveys the orbital orientation

ml

Which quantum value conveys the spin orientation

ms

Compounds made from a metal + non-metal

ionic

Ionic compounds ___ (share/transfer) electrons

transfer

Compounds made from a non-metal + non-metal

covalent

Covalent compounds ___ (share/transfer) electrons

share

Ionic compounds have ___ (high/low) melting/boiling points

high

Covalent compounds have ___ (high/low) melting/boiling points

low

___ compounds are soluble in water and conduct electricity

ionice

___ compounds are insoluble in water and do not conduct electricity

covalent

Ionic compounds have a ___ (big/small) electronegativity difference

big

Covalent compounds have a ___ (big/small) electronegativity difference

small

Increase in bond order = ___ in bond length

decrease

Dipole-dipole IMF are found in all ___ molecules

polar

Ion-dipole IMF are found in all ___ molecules

ionic and polar

Increasing IMF = ___ melting/boiling points

increasing

Increasing IMF = ___ viscosity

increasing

Increasing IMF = ___ surface tension

increasing

Increasing IMF = ___ vapor pressure

decreasing

List the strength of IMF from strongest to weakest

ion dipole, Hydrogen bonding, dipole dipole, london dispersion forces

Formal charge formula =

valence electrons - lone pairs - bonds

Metals are generally solid at room temperature except for ___, which is a ___

Hg, liquid

Non-metals are generally gas or solid at room temperature except for ___, which is a ___

Br, liquid

Metals have ___ (high/low) melting/boiling points

high

Non-metals have ___ (high/low) melting/boiling points

low

Metals are ___ (good/poor) heat conductors

good

Non-metals are ___ (good/poor) heat conductors

bad

Energy needed to remove an electron from an atom

ioniziation energy

Ionization energy increases

up and right

For ionization energy, group 2 is ___ (greater than/less than/equal to) group 13

greater than

For ionization energy, group 15 is ___ (greater than/less than/equal to) group 116

greater than

The second ionization energy is generally ___ (higher/lower) than the first ionization energy

higher

Amount of positive charge experienced by an electron

effective nuclear charge

Z_eff increases

up and down

Z_eff =

Z-S

The ability to attract an electron

electronegativity

Electronegativity increases

up and right

Atomic radius increases

down and left

Amount of energy released when an electron is added to an atom

electron affinity

Electron affinity increases

up and right