exam-1-study-guide-all-lectures-for-exam-1

c = 3.00 × 10^8 m/s.

h = 6.626 × 10^−34 J/s.

Milli.

High frequency (ν) corresponds to high energy (E).

They indicate the precision of a measurement.

To convert units from one system to another.

Higher charge results in a smaller radius in the same row/period.

It is quantized.

The result carries the same number of decimal digits as the number with the least decimal places.

Mole (mol).

Meter (m), Kilogram (kg), Second (s).

The distance between identical points on successive waves.

Kelvin (K).

6.022 x 10^23.

The number of wave cycles that occur in 1 second (Hz).

The value of l.

Spherical shape.

The radius decreases due to reduced electron-electron repulsions and a stronger pull from the nucleus.

Ionization energy increases.

The shape of the orbital.

The mass of atoms and other similar sized objects.

Newton (N).

1s < 2s < 3s (increasing size).

P = F / L².

Tera (10^12).

Add or subtract the exponents.

Energy cannot be created nor destroyed; the total amount of energy in a system does not change.

Ambiguous; it can have 2, 3, or 4 significant figures depending on context.

Values range from 0 to 3.

Mega.

The probability is 0.

D = m/v (density equals mass divided by volume).

Femto (10^-15).

Change in energy that results when force is exerted over distance.

In atomic mass units (amu).

Accuracy is how close to the actual value, while precision is consistency in measurements.

Ionic bonds typically form between metals and nonmetals.

Shape: dumbbell; l=1.

1s² 2s² 2p⁶ 3s¹.

Electrons are added to the lowest energy orbitals first before moving to higher energy orbitals.

By removing electrons first from the shell with the highest value of n.

Possible energy states of electrons.

A method that uses conversion factors to relate different physical dimensions, such as mL to grams.

An orbital can have at most two electrons with opposite spins.

The radius of a cation or anion.

In pascals (Pa).

They are extremely stable with a full outer shell.

To write very large and very small numerical values easily.

E < 0; energy is released, indicating an exothermic process.

Properties that do not depend on the amount of matter, such as temperature and density.

Because of sublevel splitting, 4s is lower in energy than 3d.

The physical state changes but the chemical identity remains the same.

Atom.

All samples of a given compound have the same proportions of their elements.

The nucleus contains most of the atom's mass.

The result contains the least amount of significant figures from the numbers involved.

Speed of wave = λ × ν.

Energy is proportional to its frequency (E photon = hv = hc/λ).

F = ma, where 'a' is acceleration.

It varies with wavelength.

101325 Pa.

The energy associated with the addition of one electron to an atom in the gas phase.

Properties that depend on the amount of matter, such as mass, volume, and energy.

Ionization energy increases going up a group.

A property that cannot be observed without changing the identity of the substance.

Half the distance between adjacent nuclei connected by a chemical bond.

1 node.

1s² 2s² 2p⁶ 3s² 3p⁵.

A condition where there is one or more unpaired electrons.

Electrons that are farther from the nucleus and involved in chemical bonding.

Matter with a definite and constant composition and distinct properties.

A property measured and expressed with numbers.

The electron is in the 1s orbital.

The frequency below which no electrons are emitted.

The size of the orbital.

An atom.

Because it connects physical sciences with life sciences.

K = °C + 273.15.

To denote multiples or fractions of base units.

1 cal = 4.184 J.

The total number of protons and neutrons in an atom.

It is impossible to know both the momentum and position of a particle simultaneously.

It is easier to add an electron to an s orbital than to a p orbital.

It is proportional to the square of the wave function (Ψ).

The energy associated with the formation of a crystal lattice from gaseous ions.

Ions are usually arranged in a crystal lattice.

ml = -2, -1, 0, 1, 2; indicating 5 orientations.

[Ar] 3d⁵.

The actual magnitude of positive charge experienced by an electron in an atom.

Elements and Compounds.

They are intermediate between metals and nonmetals.

Constructive (adding waves in phase) and Destructive (adding waves out of phase).

The number of emitted electrons increases.

Any nonzero number is significant; zeros between nonzero numbers are significant; zeros to the left of the first nonzero are not significant; zeros to the right of the last nonzero are significant if there is a decimal.

The vertical distance from the midline to the top of the peak or bottom of the trough.

Anything that has mass and occupies space.

Mass is the amount of matter present, while weight is the gravitational pull on an object.

R = 1.0973 x 10^7 m⁻¹.

In Joules (J).

The wavelength corresponding to the photon absorbed when an electron moves from a lower to a higher energy level.

Kinetic, Potential, and Radiant energy.

A substance made up of two or more elements combined in a ratio held together by chemical bonds.

Defined values, such as 1 dozen or 1 kg = 1000 g.

A covalent bond is the sharing of electrons between two atoms, typically formed between nonmetals.

As the distance between ions increases, lattice energy decreases.

A metal becomes a cation and a nonmetal becomes an anion, forming a neutral compound.

1s² 2s² 2p⁶ 3s² 3p⁶; it gains one electron and is isoelectronic with Ar.

Number of orbitals = n².

Atoms that are connected to one another.

As metals, nonmetals, or metalloids.

Group 8A elements: He to Rn.

The energies of the atomic orbitals in a shell are split.

The excess energy is converted to kinetic energy.

The radius increases due to increased electron-electron repulsions.

The number of protons in the nucleus.

The minimum energy required to remove a single electron from an atom in the gas phase.

It increases from left to right, making it easier to add an electron.

6.022 x 10^23, representing the number of elementary entities in one mole.

Nonmetals vary in color and are not shiny.

ml = -1, 0, 1; indicating 3 orientations.

Shape: complex; l=2.

The most stable arrangement of electrons is the one in which the number of electrons with the same spin is maximized.

Chromium and Copper, which have configurations [Ar] 4s1 3d5 and [Ar] 4s1 3d10 respectively.

Solid, Liquid, and Gas.

Different forms of the same element bonded differently, like Ozone (O3) and Oxygen Gas (O2).

F to At.

The wavelength.

It occurs when atoms or molecules absorb energy and release it as light energy.

They emit radiation.

S- has the largest radius.

Brittle materials are not malleable, poor conductors of heat and electricity, and have high electron affinities.

The behavior of quantum particles such as electrons and protons.

Metals are shiny, malleable, ductile, and good conductors of heat and electricity.

The mass in grams of one mole of a substance.

A = Z + N, where N is the number of neutrons.

Because they can have varying numbers of neutrons.

Using the formula n - 1, where n is the principal quantum number.

Inner shell electrons.

Volume remains the same, but shape changes.

Compounds with the same chemical formula but different structures.

How electrons are distributed in various atomic orbitals.

Light hits certain metals and emits electrons.

Emissions at different wavelengths.

Two or more species with identical electron configurations but different nuclear charges.

Observation based → description.

Meaningful digits in a reported figure.

The transfer of electrons from one atom to another and the electrostatic interaction between oppositely charged ions.

The amount of a substance that contains as many elementary entities as there are atoms in exactly 12 g of carbon-12.

The chemical identity changes.

Matter is neither created nor destroyed.

9 orbitals.

Z_eff increases from left to right because core electrons remain the same while Z increases.

A physical combination of two or more substances.

A property described using words, not numbers.

It is considered excited.

As a beam of light being a stream of energy called photons.

Ionization energies increase because the atom does not want to lose its core electrons.

All particles have a wavelength that is inversely proportional to their momentum.

Ionization energy decreases going down a group.

A property that can be observed and measured without changing the identity of the substance.

Half the distance between the nuclei of two adjacent metal atoms.

Increases top to bottom and decreases left to right.

1s² 2s² 2p⁶; it loses one electron and is isoelectronic with Ne.

2 nodes.

[Ar] 3d³; it is paramagnetic.

Transition metals and inner transition metals exhibit trends that differ from s-block elements.

A mixture that can be separated, like a salad.

Be to Ra.

When a solid is heated and emits electromagnetic radiation.

The photon is unable to dislodge the electron.

It describes the wave behavior of quantum particles.

The probability of finding an electron at a certain distance.

Using the molar mass as a conversion factor.

It has an equal number of protons and electrons.

The ratio of the two mass ratios can be expressed as small whole numbers.

All elements except hydrogen and helium.

The 2s orbital penetrates more deeply into the 1s orbital than the 2p orbital.

A mixture with a uniform composition, like vodka.

Li, Na, K, Rb, Cs, Fr.

No two electrons can have the same four quantum numbers in one atom.

W = hv, where v is the speed.

Gallium (Ga) and Germanium (Ge).

It retains shape and volume.

Good conductors, malleable, and ductile.

Rare earth metals.

s, p, d, f.

Photons that have a continuous spectrum of wavelengths.

Rows in the periodic table.

It takes the shape and volume of its container.

Poor conductors and gaining electrons in reactions.

Diffraction.

The speed of electrons increases.

To describe the wavelengths of light emitted by hydrogen.