Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry 1 > Chapter 5: Electronic Structure and Periodic Properties > Flashcards

Chapter 5: Electronic Structure and Periodic Properties Flashcards

You may prefer our related Brainscape-certified flashcards:
Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards Periodic Table flashcards
1
Q

What is ionization energy?

A

The energy required to remove one electron from an atom

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

The stability of an orbital can be determined by measuring?

A

The amount of ionization energy

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

True or False: It is easy to remove an electron from a positive species?

A

False

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

What is the screening effect?

A

The electron-electron repulsion canceled by the attraction to the nucleus

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

Electrons are only screened by____electrons?

A

Inner

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

True or False: The higher the value of the quantum number n, the more that orbital is screened by electrons in smaller, more stable orbitals?

A

True

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

True/False: the higher the value of l, the less that orbital is screened by electrons in smaller, more stable orbitals?

A

False

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

What factors control the energy of an orbital for most atoms?

A

The size and shape of the orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Do the columns of elements contain similar chemical properties?

A

Yes

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

What is the Pauli Exclusion Principle?

A

Each electron has a unique set of four quantum numbers; no two electrons can have the same set

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

What is the Aufbau Principle?

A

The placement of electrons in orbitals starting with the lowest energy orbital

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

What are the rules of Ground-State configurations?

A
  1. Each electron occupies the most stable available orbital
  2. No two electrons can have the same quantum numbers
  3. Shell capacities : s: 2 electrons
    p: 6 electrons
    d: 10 electrons
    f: 14 electrons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Accessible electrons are also called?

A

Valence electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is Hund’s rule?

A

The most stable configuration is the one with the maximum number of electrons with the same spin orientation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is noble gas configuration?

A

Specify the noble gas before the element and then write the remaining configuration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What two elements don’t follow the regular progression of configuration? What is their configuration?

A

Cr: 4s1 3d5
Cu: 4s1 3d10

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What are near-degenerate orbitals?

A

Orbitals with nearly the same energy. Because the orbitals are so close in energy, it is possible for an electron to the promoted to the higher energy level

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Isoelectronic

A

Atoms and ions that have the same number of electrons

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

For neutral atoms and anions, place electrons in _____ before ________

A

ns, (n-1)d

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

For cations, place electrons in _____before_____

A

(n-1)d, ns

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

Paramagnetic

A

Attracted to a magnet, aligns itself in a magnetic field

18
Q

Diamagnetic

A

Repelled by a strong magnet

19
Q

Are paramagnetic materials weak or strong?

A

Weak

20
Q

Strong paramagnetic materials are called

A

Ferromagnetic

21
Q

The number of unpaired electrons in a paramagnetic substance can be measured with a____

A

Gouy balance

22
Q

What type of substance does paramagnetism occur in?

A

Ions or atoms with unpaired electrons

22
Q

What type of substance does diamagnetism occur in?

A

Ions or atoms that have paired electrons

23
Q

Atomic radii

A

The distance between the nucleus and outer surface of the largest orbital

24
Q

Electron affinity

A

The energy change when an electron is added to an atom

24
Q

Ionization energy

A

Energy required to remove an electron from an atom in the gas phase

25
Q

As n increases, atomic orbitals____

A

Become larger and less stable

26
Q

As Z increases, atomic orbitals____

A

Become smaller and more stable

27
Q

What is Z?

A

Atomic number (number of protons)

28
Q

For the main group elements, the ionization energy increases___?

A

Going up and across the right of the periodic table

29
Q

Does electron affinity have a clear trend as n increases? What is the one general pattern?

A

No. Electron affinity tends to become more negative moving from the left to right across a row of the periodic table

29
Q

Zeff increases as the number of electrons____?

A

Decreases

As the number of electrons decrease, each electron feels a greater electrical attraction to the nucleus, resulting in a larger ionization energy

30
Q

What are the irregularities in ionization energies?

A
  1. Aluminium has a smaller ionization energy than either of its neighbours in Row 3
  2. Oxygen has a smaller ionization energy than either of its neighbours in Row 2.
31
Q

The radius of a cation is always____than the corresponding atom

A

Smaller

32
Q

The radius of an anion is always ______ than the corresponding atom

A

Larger

33
Q

For isoelectronic species, as Z increases __________?

A

It becomes more difficult to remove an electron

34
Q

What is the vaporization and ionization of an atom to form a cation?

A

(s) —–> (g) + e-

Esublimation= (+)
E=IE= (+)

35
Q

Condensation of the two to form the solid salt

A

(+) + (-) —-> (s)

(-)E lattice = (-)

35
Q

Bond breakage and ionization of atom to form an anion

A

(g) + e- ——> -(g)

E=1/2BE= (+)
E=EA= (-)

36
Q

Overall reaction

A

Add all of the energies together

37
Q

What is the Born-Haber cycle?

A

A series of steps involving ions in the gas phase

38
Q

What is lattice energy?

A

The energy released when an ionic solid decomposes into gaseous ions

39
Q

What does the magnitude of lattice energy depend on?

A

The charges of the ions, their size, and lattice arrangement

39
Q

Are ions formed by removing core electrons found in stable ionic compounds?

A

No

40
Q

What are halides?

A

When halogens react with metals to form binary compounds. They contain metal cations and halide anions

40
Q

Isolated atomic anions with charges more negative than -1 are always unstable except for _____?

A

O2- and S2-

41
Q

What are the trends in lattice energy?

A
  1. Lattice energy will increase as ionic charge increases and will decrease as ionic size increases
  2. Lattice energy is the sum of all ion interactions in the solid ionic compound

Chemistry 1 (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions