DAT FLASHCARDS QUESTIONS AND
ANSWERS WITH SOLUTIONS 2024
# orbitals per shell - ANSWER n²
# electrons per shell - ANSWER 2n²
# electrons in SUB SHELL - ANSWER 4l + 2
l= angular momentum - ANSWER range: 0 to (n-1)
m= magnetic quantum number - ANSWER range: -l to +l
Aufbau Principle - ANSWER Shells/ sub shells of lowest energy get filled first
Hund's Rule - ANSWER Add electrons to orbitals with single electron and with same spin--> electrons
prefer to singly occupy an orbital and more favorable to spin in same direction
Pauli Exlcusion Principle - ANSWER 2 electrons in same orbital must be of different spins
Electron configuration TRAP - ANSWER d⁴ and d⁹, they prefer to have d either full or half filled and have s
half filled
Shielding electrons on Bohr model - ANSWER Shielding e's are those that orbit at smaller radius (than
valence)
Alkali Metals - ANSWER - Group I elements
- Very reactive
- Forms oxides with oxygen
- Forms hydroxides with water--> releases H+
,- Reacts with acids to form salts---> releases H+
Alkaline Earth Metals - ANSWER - Group II
- Wants to lose both valence e's
- Forms oxides with oxygen and hydroxides with water
- Reacts with acids and forms salts--> releases H+
Halogens - ANSWER - Forms salts with Groups I and II
- Usually -1 oxidation state
- F is most eneg
Electronegativity Mnemonic - ANSWER - F rogs
- O ften
- Cl ing
- N ear
- Br anches
-In
- S wampy
- C onditions
- H owever
- P arrots
- B oldly
- Si ng
- Al oud
Noble Gases - ANSWER - High IE and low EA
- Don't react
- Oxidation state= 0!
,Transition metals - ANSWER - D block
- High conductivity due to loosely bound outer d electrons
- Complex with ligands and d orbitals change in energy (nondegenerate)
- Electron transitions between nondegenerate d orbits gives transition metal complexes vivid colors
- Always have a POSITIVE oxidation #
Representative elements - ANSWER - S and P block
- DOES NOT include the d block
- No loosely bound d electrons
Metalloids - ANSWER - 5 elements in line from B to At (BAT) and Ge and Sb
- In between metals and nonmetals in character
Metals - ANSWER - Likes to LOSE e's an gain + charge
- More electroPOSITIVE
- Forms basic oxides
- Good heat and electricity conductor
- Malleable, ductile, luster
- Solid at room temp except Hg which is liquid
- GOOD REDUCING AGENTS (ie. they like to be oxidized!)
Non Metals - ANSWER - GOOD OXIDIZING AGENTS (like to be reduced!_
- Like to GAIN electrons (high eneg)
- More electronegative
- Forms acidic oxides
- Bad heat and electricity conductor
- Solid, l, or gas at room temp
- If solid, brittle and not shiny
, Ionization Energy - ANSWER - amount of energy needed to knock off first valence electron
- Increases from L to R
- Increases from Bottom to Top
- 2nd IE ALWAYS higher than 1st IE due to e-e repulsion
- Highest peaks are noble gases
- Lowest troughs are alkali metals
Electron Affinity - ANSWER - amount of energy RELEASED when something gains an electron
- Increases from bottom to top and left to right
- Peaks= halogens
- Troughs= noble gases
Atomic radius - ANSWER - Decreases left to right
-Increases top to bottom
- Influenced by Zeff and electrostatic attraction between nucleus and electrons
- Higher Zeff means more attraction and atom becomes more compact
- Peaks= single electron in valence ( Li, Na, K)
- Troughs= Noble gases (totally filled shell)
Ions and radius size - ANSWER - Positive ions are SMALLER than parent atom (fewer shielding electrons
and stronger force felt on electrons by nucleus)
- Negative ions are LARGER--> they have more shielding e's and more e-e repulsion so radius expand
Lattice energy - ANSWER - LE measures ionic bond strength
- LE is the energy required to BREAK ionic bond
- LE α electrostatic attraction between ions
Electrostatic force - ANSWER F= kQQ/ r²
ANSWERS WITH SOLUTIONS 2024
# orbitals per shell - ANSWER n²
# electrons per shell - ANSWER 2n²
# electrons in SUB SHELL - ANSWER 4l + 2
l= angular momentum - ANSWER range: 0 to (n-1)
m= magnetic quantum number - ANSWER range: -l to +l
Aufbau Principle - ANSWER Shells/ sub shells of lowest energy get filled first
Hund's Rule - ANSWER Add electrons to orbitals with single electron and with same spin--> electrons
prefer to singly occupy an orbital and more favorable to spin in same direction
Pauli Exlcusion Principle - ANSWER 2 electrons in same orbital must be of different spins
Electron configuration TRAP - ANSWER d⁴ and d⁹, they prefer to have d either full or half filled and have s
half filled
Shielding electrons on Bohr model - ANSWER Shielding e's are those that orbit at smaller radius (than
valence)
Alkali Metals - ANSWER - Group I elements
- Very reactive
- Forms oxides with oxygen
- Forms hydroxides with water--> releases H+
,- Reacts with acids to form salts---> releases H+
Alkaline Earth Metals - ANSWER - Group II
- Wants to lose both valence e's
- Forms oxides with oxygen and hydroxides with water
- Reacts with acids and forms salts--> releases H+
Halogens - ANSWER - Forms salts with Groups I and II
- Usually -1 oxidation state
- F is most eneg
Electronegativity Mnemonic - ANSWER - F rogs
- O ften
- Cl ing
- N ear
- Br anches
-In
- S wampy
- C onditions
- H owever
- P arrots
- B oldly
- Si ng
- Al oud
Noble Gases - ANSWER - High IE and low EA
- Don't react
- Oxidation state= 0!
,Transition metals - ANSWER - D block
- High conductivity due to loosely bound outer d electrons
- Complex with ligands and d orbitals change in energy (nondegenerate)
- Electron transitions between nondegenerate d orbits gives transition metal complexes vivid colors
- Always have a POSITIVE oxidation #
Representative elements - ANSWER - S and P block
- DOES NOT include the d block
- No loosely bound d electrons
Metalloids - ANSWER - 5 elements in line from B to At (BAT) and Ge and Sb
- In between metals and nonmetals in character
Metals - ANSWER - Likes to LOSE e's an gain + charge
- More electroPOSITIVE
- Forms basic oxides
- Good heat and electricity conductor
- Malleable, ductile, luster
- Solid at room temp except Hg which is liquid
- GOOD REDUCING AGENTS (ie. they like to be oxidized!)
Non Metals - ANSWER - GOOD OXIDIZING AGENTS (like to be reduced!_
- Like to GAIN electrons (high eneg)
- More electronegative
- Forms acidic oxides
- Bad heat and electricity conductor
- Solid, l, or gas at room temp
- If solid, brittle and not shiny
, Ionization Energy - ANSWER - amount of energy needed to knock off first valence electron
- Increases from L to R
- Increases from Bottom to Top
- 2nd IE ALWAYS higher than 1st IE due to e-e repulsion
- Highest peaks are noble gases
- Lowest troughs are alkali metals
Electron Affinity - ANSWER - amount of energy RELEASED when something gains an electron
- Increases from bottom to top and left to right
- Peaks= halogens
- Troughs= noble gases
Atomic radius - ANSWER - Decreases left to right
-Increases top to bottom
- Influenced by Zeff and electrostatic attraction between nucleus and electrons
- Higher Zeff means more attraction and atom becomes more compact
- Peaks= single electron in valence ( Li, Na, K)
- Troughs= Noble gases (totally filled shell)
Ions and radius size - ANSWER - Positive ions are SMALLER than parent atom (fewer shielding electrons
and stronger force felt on electrons by nucleus)
- Negative ions are LARGER--> they have more shielding e's and more e-e repulsion so radius expand
Lattice energy - ANSWER - LE measures ionic bond strength
- LE is the energy required to BREAK ionic bond
- LE α electrostatic attraction between ions
Electrostatic force - ANSWER F= kQQ/ r²
