Got wrong Flashcards
Electron cloud
Consists of high energy electrons existing in energy shells
Ion
A charged particle that is formed when an atoms gains or loses electrons from its outer shell
1s² 2s² 2p⁶ 3s¹
What do the 1, 2 and 3 Infront mean
Shell Number
1s² 2s² 2p⁶ 3s¹
What do the s and p’s mean
Subshell that is being filled
1s² 2s² 2p⁶ 3s¹
What do the ² ⁶ ¹
Number of electrons in subshell
Hund’s Rule
Every Orbital in a subshell is singly occupied being any orbital is doubly occupied
Shell vs subshell vs orbital
Shells are broad energy levels.
Subshells are divisions within shells that group orbitals of similar energy.
Orbitals are specific regions in a subshell where electrons exist.
How many electrons can orbitals hold
2
Number of orbitals in s-subshell
1
Number of orbitals in p-subshell
3
Number of orbitals in d-subshell
5
Number of orbitals in f-subshell
7
What is the maximum number of electrons in a shell
2𝑛²
Shells
Shells:
Shells are the major energy levels in an atom.
They are represented by the principal quantum number 𝑛 (e.g., 𝑛 = 1, 2, 3 etc)
The maximum number of electrons a shell can hold is determined by the formula 2𝑛²
Subshells
Each shell is divided into subshells of similar energy.
Subshells are labeled s, p, d, and f.
Each type of subshell has a different maximum number of electrons:
s-subshell: 2 electrons
p-subshell: 6 electrons
d-subshell: 10 electrons
f-subshell: 14 electrons
Orbitals
Orbitals are the regions within a subshell where electrons are most likely to be found.
Each orbital can hold a maximum of two electrons.
The number of orbitals in each subshell is as follows:
s-subshell: 1 orbital (holds 2 electrons)
p-subshell: 3 orbitals (each holding 2 electrons, total 6)
d-subshell: 5 orbitals (each holding 2 electrons, total 10)
f-subshell: 7 orbitals (each holding 2 electrons, total 14)
Anion
Negative ion formed when non-metal atoms gain electrons to match the number of valence e⁻ of their nearest noble gas.
Cation:
positive ion formed when metal atoms lose e⁻ to match the number of valence e⁻ of their nearest noble gas.
Diatomic molecules:
where two atoms of the same element share e⁻.
Ion
A charged particle
Polyatomic ion
A polyatomic ion is an ion composed of two or more atoms that are covalently bonded and function as a single charged entity.
Equation of Cation for H
H -> H⁺ + e⁻
Equation of Anion for F
F + e⁻ -> F⁻
Naming of ionic compounds
Metal followed by non-metal
no extra prefixes
Metal -> Original name
Non - metal -> “-ide” suffix
What is a dipole
A dipole is the separation of charge in a molecule due to differences in electronegativity. One end becomes partially positive (δ⁺), and the other partially negative (δ⁻).
Types:
Permanent Dipole: Found in polar molecules (e.g., HCl, H₂O).
Instantaneous/Induced Dipole: Temporary charge shifts (e.g., London dispersion forces).
Naming of Covalent compounds
First non-metal has original name, 2nd ends in “__ide”
Prefixes
Mono - (Only for 2nd non metal)
Di
Tri
Tetra
Penta
Hexa
Hepta
Oct
Non
Dec
Polar bonds in covalant compounds
If the electronegativities of the two atoms are very different, than the electron pair will tend toward the more negative of the two atoms
Non-polar bonds in covalent compounds
Occurs between two atoms that are the same or have similar electronegativity
Covalent network solids
Some elements mainly ( C and Si) Some elements (mainly C & Si) can form 4 covalent bonds with other elements (C & Si) to create a network (lattice) solid.
These networks are
very strong & hard
have very high melting points
Do not conduct electricity
What does metals being malleable and ductile tell you about their structure
The attraction forces between the particles must be stronger than the repulsive forces when the layers are moved
How to represent isotopes
Nuclear Notation (or Standard Isotopic Notation) → ᴬX
Example: ¹⁴C (Carbon-14)
Hyphen Notation - X-A
Example: Carbon-14
How does mass spectroscopy work
1: Sample is vaporized
2: Ion accelerated through electric field
3: Fast moving ions separated by a magnetic field
Graph of Mass spectrometer:
What the number of peaks tells us:
What the position of peaks tells us:
What the height of peaks tells us:
Number of isotopes
Relative isotopic mass
Relative abundance of the isotope (in comparison to other isotopes of that element)
What is m / z
m/z (mass-to-charge ratio) is the ratio of an ion’s mass (𝑚) to its charge (𝑧). It determines the position of peaks in a mass spectrum and helps identify molecules.
