General Chemistry Midterm: Chapter E-5.4

Compounds

When more than one element combines, they form this. (an element mixture)

SI Units

Based on the metric system.

Length

What is the unit “meter” used to measure?

Mass

What is the unit “Kilogram” used to measure?

Time

What is the unit “Second” used to measure?

Amount of Substance

What is the unit “Mole” used to measure?

Round it to the right number of Significant figures.

What can be done in order to make the number more precise?

mL or cm³

What units can Volume be written as?

The principal quantum number

What is the n symbolizes?

It symbolizes the angular number and tells us whether it is a s, p or d orbital.

What does the l symbolize and what does it tell us?

You find the number of radial nodes by looking at where the graph touches the x-axis.

How do you find the number of radial nodes?

They go from a high energy state to a low energy state.

How do electron configurations work?

When an electron goes from a high to a low energy state.

What is an Emission in an energy state change?

Going from a lower energy state to a higher energy state

What is an Absorption in an energy state change?

When electrons are unpaired and attracted to an external magnetic field.

What is a paramagnetic electron configuration?

Yes

Do electrons get ejected when there is more energy?

No

Do electrons get ejected when there is a low frequency?

It is the inverse of energy - if there is a lower wavelength there is a higher energy

What is wavelength’s relationship to energy?

Pauli Exclusion Principle

When 2 electrons in the same species cannot have all four quantum numbers be equivalent. (Arrows cannot be equivalent in a s or p subshell)

Hund’s Rule

every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Aufbau Principle

This means that you have to start from the lowest energy state to the highest energy state.

Boron's size and high nuclear charge cause it to behave differently than other elements- Plus Boron’s 2s orbital is filled so their orbitals are more stable

Why is there an anomaly in the Boron and Beryllium element?

Nitrogen’s orbital is filled- making it more stable while Oxygen has half filled orbitals, causing electron electron replusion.

Why is there an anomaly in the Oxygen and Nitrogen element?

They want to lose electrons.

What are metal’s valence electrons like?

They want to get more stable.

What are nonmetal’s valence electrons like?

2+

What are the charges for Zn and Cd?

Cu, Ag, Au, Cr, and Mo

What are the elements that have abnormal electron configurations?

They lower it.

What does chemical bonding do to the potential energy of the atoms or ions that are bound together?

Covalent Bonding

When elements (nonmetals) share electrons.

Ionic Bonds

When metals and nonmetals transfer electrons.

More energy is released.

What happens in all chemical bonds?

It would be Polar Covalent

If the distance in a dipole moment is long, what does that mean for the bond? (Along with electronegativity difference)

Releasing energy

What does exothermic mean?

Energy entering

What does endothermic mean?

Pauling electronegativity

This is based on each element bonding to other elements. (bond strength, bond weakening, etc.)

Si-H and C-H

What are the 2 bonds that are NONPOLAR COVALENT

H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂

What are the 7 diatomic molecules?

nanometers

What are the units used in wavelength?

Joules (sometimes eV if they ask for it)

What are the units used for Eₚₕₒₜₒₙ?

The bond strength weakens.

If the bond length increases, what happens to the bond strength?

It gets stronger.

If the bond length decreases, what happens to the bond strength?

They have high nuclear charge yet are low in energy.

What is a characteristic of a core electron?

they have low nuclear charge but they are high in energy.

What is a characteristic of valence electron?

Ionic Bonds

A bond formed between a metal and a nonmetal where electrons are not equally shared and they are transformed from one atom to another.

Covalent Bonds

Bonds formed between 2 nonmetals where valence electrons are shared between one another.

Chemical bond

The force that holds atoms together in a compound.

They lower the potential energy of the charged particles that compose atoms.

Why do chemical bonds form?

The one with the lowest potential energy.

What compound would be the most stable one?

Mono-

What is the Greek prefix for 1?

Di-

What is the Greek prefix for 2?

Tri-

What is the Greek prefix for 3?

Tetra

What is the Greek prefix for 4?

Penta

What is the Greek Prefix for 5?

Hexa-

What is the Greek Prefix for 6?

Hepta

What is the Greek Prefix for 7?

Octa

What is the Greek Prefix for 8?

Nona

What is the Greek Prefix for 9?

Deca

What is the Greek Prefix for 10?

Transition Metals

What type of metals will have Roman numbers in front of their name?

Acetate

CH₃COO⁻

Carbonate

CO₃²⁻

Bicarbonate ( hydrogen carbonate )

HCO₃⁻

Nitrate

NO₃⁻

Nitrite

NO₂⁻

Sulfate

SO₄²⁻

Sulfite

SO₃²⁻

Phosphate

PO₄³⁻

Hydrogen Phosphate

HPO₄²⁻

Dihydrogen Phosphate

H₂PO₄⁻

Oxalate

C₂O₄²⁻

Cyanide

CN⁻

Chromate

CrO₄²⁻

Dichromate

Cr₂O₇²⁻

Permangnate

MnO₄⁻

Peroxide

O₂²⁻

Azide

N₃⁻

Per- -ate

XO₄⁻

-ate

XO₃⁻

-ite

XO₂⁻

Hypo- -ite

XO⁻

Ammonium

NH₄⁺

Hydroxide

OH⁻

Hydronium

H₃O⁺

Pb (Lead) and Sn (Tin)

Which 2 elements would need Roman numerals in front of their compound names?

Chromium

Electron Configuration: [Ar] 3d⁵ 4s¹

Copper

Electron Configuration: [Ar] 3d¹⁰ 4s¹

Niobium

Electron Configuration: [Kr] 4d⁴ 5s¹

Molybdenum

[Kr] 4d⁵ 5s¹

Ruthenium

Electron Configuration: [Kr] 4d⁷ 5s¹

Rhodium

Electron Configuration: [Kr] 4d⁸ 5s¹

Palladium

Electron Configuration: [Kr] 4d¹⁰ 5s⁰

Silver

Electron Configuration: [Kr] 4d¹⁰ 5s¹

Lanthanum

Electron Configuration: [Xe] 5d¹ 6s²

Actinium

Electron Configuration: [Rn] 6d¹ 7s²

Thorium

Electron Configuration: [Rn] 6d¹ 7s²

The ones within the same group and the same valence electrons.

What 2 elements would be more similar?

9.11E-31

What is the mass of an electron?

-1.602E-19 (e) 1.602E-19 (p)

What is the charge for either an electron or a proton?

3.336E-30

What unit would be used to convert dipole length?

4s

Which energy state is lower in this case: 4s or 4p?