Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Honors Chemistry > Test 3 > Flashcards

Test 3 Flashcards

(52 cards)

Start Studying
1
Q

how can you tell valence electrons from the periodic table?

A

group

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

how can you tell the number of shells from the periodic table?

A

period

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Orbitals and orientations (there can be two electrons in each orientation)

A

Spherical - 1
Peripheral - 3
Diffuse - 5
Fundamental - 7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Orbital

A
  • also known as an orientation

- a “pocket” within the subshell that can hold up to 2 electrons of different spin

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Aufbau Principle

A

At ground state, electrons must have the lowest possible energies

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Pauli exclusion principle

A

If n, l, and ml are the same for two electrons, they must have different ms (or spin)
-If a box already has an arrow, the second arrow must point in the opposite direction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Hund’s rule

A
  • orbitals within a subshell have equivalent energy, and since electrons repel, they spread out through out the orbitals as much as possible
  • Because electrons repel each other, they spread out until they no longer can
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

how many orbitals and electrons can fit in the s subshell?

A

1-2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

how many orbitals and electrons can fit in the p subshell?

A

3-6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

how many orbitals and electrons can fit in the d subshell?

A

5-10

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

how many orbitals and electrons can fit in the f subshell?

A

7-14

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

principle quantum number

A
  • n
  • the number of shells
  • n = 1,2,3 etc..
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

angular momentum quantum number

A
  • l
  • The subshell
  • l = 0,1,2,3 for s, p, d, and f respectively
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

magnetic quantum number

A
  • ml
  • tells the orbital
  • 1,0 +1
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

slit screen experiment

A

-showed that electrons must be spinning because sometimes they are attracted to the magnet. Whether an electron has an up or down spin is completely random. IF one electron in an orientation changes, the other must change as well.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

spin quantum number

A
  • ms
  • ms = +1/2 up
  • ms = -1/2down
  • when something is spinning and it hits something, its spin will determine whether it deflects to the right or to the left
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

paramagnetism

A

a weak attraction to a magnetic field

-occurs when there are one or more unpaired electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

diamagnetism

A
  • weak repulsion from a magnetic field

- occurs when all electrons are paired

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

two forms of stability

A
  • having the lowest possible energy

- having exactly filled or half-filled subshells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

however, having lowest possible energy in order to be stable breaks down in the transition metals because….

A

sometimes, an electron will move up a level (breaking the principle) to further stabilize an atom by having either a filled or half-filled subshell for the valence electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

levels of stability (even charge distribution leads to the most stability

Study These Flashcards
A
  • most stable: full s and p
  • stable: full subshells in general
  • medium stable: exactly half-filled subshells
  • not particularly stable: anything else
22
Q

transition metals

Study These Flashcards
A
  • have incompletely filled d subshells, and will readily lose electrons to try to stabilize
  • Form cations (although they will not be quite isoelectronic with a noble has, they will have full s and p subshells like a noble gas
23
Q

ionic reaction

Study These Flashcards
A

any time something loses/gains electrons
-happens because every participating atom either loses or gains electrons ignored to become isoelectronic with a noble gas

24
Q

atomic radius

Study These Flashcards
A
  • increases diagonally from the top right to the bottom left (protons decrease to the left and shells increase toward the bottom)
  • Increases in the same pattern as shielding because shielding lessens the nucleus’s ability to hold on to its electrons
  • distance from the nucleus to the valence shell (measured as 1/2 the distance between two nuclei that are bonded together
25
Electronegativity (EN)
- increases to the top right (the less shielding there is, the more electronegativity there will be) - measures how much an element will own an electron in a bond - An electron spends more time with the nucleus that is more electronegative
26
electron affinity (EA)
- Increases diagonally from the bottom left to the top right (represents how attractive a nucleus is to an electron) - Highest in the halogens. This is because the noble gases do not want to receive electrons - The energy that is released when an electron is gained (to produce an anion) - If the attraction is strong, lots of energy is released - EA and IE are basically the same thing, just with different experimental methods
27
Ionization energy (IE)
- increase diagonally from the bottom left to the top right - the energy it takes to remove an electron - we can electrocute atoms, and if there's enough energy, an electron will fly off and form a cation - it takes more energy to remove the second electron than the first and so on. The energy before the big jump is the final valence electron.
28
shielding
- electrons are attracted to the nucleus and repelled by each other - Because of repelling core electrons, outer electrons do not feel as attracted to the nucleus - proportional to the number of shells. Adding more electrons to a row does not really make a difference. In fact, it decreases shielding because across a row, number of protons increases as number of electrons increases. - Inversely proportional to the number of protons (fewer protons = more shielding towards the bottom left)
29
effective nuclear charge
Zeff - The force of attraction is inversely proportional to the distance o - Fbetween charges [fish proportional symbol] 1/ distance - Fbetween charges is proportional to the magnitude of the charge
30
force
the interaction between two charges
31
when you cross the staircase, do elements want to gain or lose electrons?
they want to gain electrons
32
covalent bond
- when the electrons in a bond are shared equally - happens among nonmetals - delta EN among non polar covalent bonds ranges from 0-0.5 - Strong bonds (not broken by melting/boiling) - Atoms have no charge
33
Polar covalent bond
- electrons are shared unequally - transfer of an electron that results in charges that attract - occurs among nonmetals that are far enough away from each other - 0.5-1.7 - Atoms have slight positive and slight negative charges
34
ionic bond
- when electrons are transferred - always happens between a metal (cation) and a nonmetal (anion) - A big difference in EN - 1.7-3.3 - Atoms have full charges - Disconnect in water - Satisfies the octet rule by transferring electrons
35
metallic bonds
- valence electrons are shared collectively, delocalized across all the nuclei - the source of a metal's strength, conductivity, and malleability
36
dative bond
if something shares a pair of electrons, and both electrons originally came from
37
octet rule
generally, all atoms will have 8 valence electrons (full s and p subshells) in the final structure
38
bonding pairs
a pair of shared electrons
39
lone pair
a pair of electrons belonging to only one atom
40
formal charge
represents how many electrons are gained or lost by an atom (valence electrons - associated electrons) - associated electrons = unshared + shared/2 - the more stable structure has more evenly distributed formal charge
41
ionic compound binary naming
- name of the metal + name of the nonmetal with -ide suffix - metal (cation) always comes before the nonmetal (anion) - If a transition metal, the charge is a roman numeral after it - if a polyatomic atom, use the collective name
42
molecular compounds
- name first nonmetal and then second nonmetal with -ide suffix (in the order of the formula) - If more than one of each type of atom, use a prefix to denote the number
43
1
mono
44
2
di
45
3
tri
46
4
tetra
47
5
penta
48
6
hexa
49
7
hepta
50
8
octa
51
9
nona
52
10
deca

Honors Chemistry (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions