Chemistry Test 2 Vocabulary Flashcards

Vocabulary flashcards covering atomic basics, waves, quantum numbers, energy transitions, and magnetic properties based on the Chemistry Test 2 study guide.

Atomic Number ($Z$)

The number of protons in an atom.

Ionization Energy

How much energy it takes to remove an electron from an atom.

Valence Electrons

Electrons with the highest energy; they determine how an element reacts.

Can be found by finding which column it is in.

Isoelectronic

Elements Having the same number of electrons.

Mole

A unit representing tiny particles.

Symbol used to represent the speed of light

$$c$$

Wavelength

$$\lambda$$

Frequency

$$\nu$$

measured in cycles/sec, $\text{s}^{-1}$, or $\text{Hz}$

($1\,\text{Hz} = 1\,\text{s}^{-1}$ ).

Photon

A particle of light representing the smallest packet of electromagnetic radiation.

Photoelectric Effect

The ejection of electrons when light hits a material with photons having sufficient energy above a threshold frequency.

Ground State

The lowest energy orbit of an electron, corresponding to $n = 1$.

What is the order of the electromagnetic spectrum (EMS)?

How is it memorized?

Radio waves, microwaves, infrared radiation, cosmic single light, ultraviolet radiation, x-rays, gamma rays.

“Red Martians Invade Venus Using X-ray Guns”

When going left to right on the EMS, what is the wave length?

Smallest, to biggest

When going left to right on the EMS, what is the frequency/energy?

Biggest, to smallest.

How do you find the photon energy?

$$E=hv$$

$$E=\frac{hc}{\lambda}$$

Rydberg equation, calculating energy change

Change in $E=R_{H}\cdot Z^2\cdot\left(\frac{1}{n^2_{f}}-\frac{1}{n^2_{i}}\right)$

Z= atomic number

Nf = final shell

Ni = initial shell

Principal Quantum Number ($n$)

The row number

Quantum number indicating energy level, shell, $1, 2, 3, 4\dots$

Angular Momentum Quantum Number ($l$)

$$0 = s$$

$$1 = p$$

$$2 = d$$

$$3 = f$$

It indicates the subshell, or known as energy.

Magnetic Quantum Number ($m_l$)

$-l$ to $+l$.

Shows orbital orientation or number of orbitals

Spin Quantum Number ($m_s$)

If the last attendant is up: $+\frac{1}{2}$

If the last arrow dean is down: $-\frac{1}{2}$

Quantum number specifying electron spin orientation

Quantum number set

(n, L, mL, ms)

Paramagnetic

an atom or ion that has unpaired electrons, making it magnetic.

Diamagnetic

an atom or ion in which all electrons are paired, making it not magnetic.

Procedure for drawing Lewis dot structures of neutral atoms

Determine the number of valence electrons from the group number.

then draw dots representing those electrons around the element symbol, placing one dot per side before pairing.

Procedure for writing condensed noble gas electron configurations

Locate the noble gas in the row above the element, then go to the far right column.

write the remaining electron configurations it takes to get from the Nobel gas to the original element.

Rules for writing electron configurations of ions

(When the element has a + or - charge to it)

For cations (positive charge), remove electrons. start from the subshell with the highest available (n)

For anions (negative charge), add electrons to the lowest available (n)

Procedure to determine if an atom or ion is paramagnetic or diamagnetic

Examine the orbital diagram or electron configuration: if there is at least one unpaired electron, it is paramagnetic; if all electrons are paired, it is diamagnetic.

When writing ms or known as arrows

Start at the beginning of each row.

The first half of sub-levels/energy levels is a up arrow.

The second half of sub-levels/energy level is a down arrow.