Brainscape's Knowledge GenomeTM

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


See full index

PIC LEC > INTRODUCTION TO INORGANIC CHEMISTRY: THE PERIODIC TABLE OF ELEMENTS > Flashcards

INTRODUCTION TO INORGANIC CHEMISTRY: THE PERIODIC TABLE OF ELEMENTS Flashcards

1
Q

DALTON’S ATOMIC THEORY

A
  1. All matter consists of atoms; tiny indivisible particles of an element that cannot be created or destroyed.
  2. Atoms of one element cannot be converted into atoms of another element.
  3. Atoms of an element are identical in mass and other properties and are different from the atoms of any other element.
  4. Compounds result from the chemical combination of a specific ratio of atoms of different elements.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

ATOMIC STRUCTURE

A
  1. Positively charged nucleus
  2. Negatively charged electrons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

(very dense,protons and neutrons) and small (10-15 m)

A

Positively charged nucleus

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

are in a cloud (10-10 m) around nucleus

A

Negatively charged electrons

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

It is impossible to know simultaneously both the momentum (mass times velocity) and the position of a particle with certainty.

A

Werner Heisenberg

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

Region of space where electron is most likely found.

A

ATOMIC ORBITALS

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

Four different kinds of orbitals for electrons:

A
  • s orbitals
  • p orbitals
  • d orbitals
  • center f orbitals
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

spherical, nucleus at center

A

s orbitals

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

dumbbell-shaped, nucleus at middle

A

p orbitals

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

elongated dumbbell-shaped, nucleus at center

A

d orbitals

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

complex, nucleus at the center

A

f orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q
  • Orbitals are grouped in shells of increasing size and energy
  • Different shells contain different numbers and kinds of orbitals
  • Each orbital can be occupied by two electrons
A

ORBITALS AND SHELLS

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

are grouped in shells of increasing size and energy

A

Orbitals

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

contain different numbers and kinds of orbitals

A

Different shells

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

Each _________ can be occupied by two electrons

A

orbital

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

(capacity - 18 electrons)

A

3rd shell

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

(capacity - 8 electrons)

A

2nd shell

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

(capacity—2 electrons)

A

1st shell

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

“Distribution of electrons”

  • Describes the number and arrangement of electrons in orbitals, subshells and shells in an atom.
A

ELECTRON CONFIGURATION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q
  • Numbers used to give information about the location of an electron in an atom with respect to its energy level, sublevel, orbital, and spin.
  • Every electron has a set of four quantum numbers.
A

QUANTUM NUMBERS

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

Numbers used to give information about the location of an electron in an atom with respect to its _________________________

A

energy level, sublevel, orbital, and spin.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Every electron has a set of ____________ numbers.

A

four quantum

23
Q

Describe the orbital occupied by an electron.

A

QUANTUM NUMBERS

24
Q

QUANTUM NUMBERS
Tells us:

A
  • Distance from the nucleus
  • Shape
  • Position
  • Spin
25
Q

4 QUANTUM NUMBERS

A
  1. Principal Quantum Number
  2. Angular Momentum Quantum Number
  3. Magnetic Quantum Number
  4. Spin Quantum Number
26
Q
  • Describes the size of the orbital
  • Indicates the main energy level (shell) surrounding the nucleus or the average distance of the electron from the nucleus.
  • The range of “n” is 1-> infinity , thus, principal quantum number (n) is always greater than 0.
A

Principal Quantum Number (n)

27
Q

size of the orbital

A

Principal Quantum Number (n)

28
Q

main energy level (shell)

A

Principal Quantum Number (n)

29
Q
  • Describes the shape or type of the orbital.
  • There are four types of orbitals: s (0) , p (1), d (2), f (3)
  • Orbitals have shapes that are best described as spherical (l = 0), polar (l = 1), or cloverleaf (l = 2).
  • For a given value of n, l has possible integral values from 0 to (n - 1).
A

Angular/Azimuthal Momentum Quantum Number (l)

30
Q

shape or type of the orbital.

A

Angular/Azimuthal Momentum Quantum Number (l)

31
Q

There are four types of orbitals:

A

s (0) ,
p (1),
d (2),
f (3)

32
Q

A collection of orbitals with the same value of n shell.

A

Shell

33
Q

One or more orbitals with the same n and l values

A

Subshell

34
Q

The orbitals in an atom are arranged in __________

A

shells and subshells

35
Q

all orbitals with the same value of n

A

Shell

36
Q

all orbitals with the same value of both n and l

A

Subshell

37
Q
  • The magnetic quantum number determines the position of electron in the orbital.
  • Consequently, its value depends on the orbital angular momentum quantum number.
  • For a certain value of l, there are (2l+1) integral values of ml
  • So Magnetic Quantum Number(ml) can be zero, a negative integer,or a positive integer.
A

Magnetic Quantum Number (ml)

38
Q

determines the position of electron in the orbital.

A

magnetic quantum number

39
Q

s sublevels contain

A

1 orbital
1 position

40
Q

p sublevels contain

A

3 orbitals
3 positions

41
Q

d sublevels contain

A

5 orbital
5 position

42
Q

f sublevels contain

A

7 orbitals
7 positions

43
Q
  • represents the direction of spin of an electron which may be either +1⁄2 (­ or spin up), or –1⁄2 ( ̄ or spin down).
  • Unlike n, l, and ml, the electron spin quantum number does not depend on another quantum number.
  • There can be a maximum of two electrons occupying any one orbital.
  • Single electrons have parallel spins and paired electrons have opposite spins
A

Spin Quantum Number (ms)

44
Q

direction of spin of an electron

A

Spin Quantum Number (ms)

45
Q

Electrons ni atoms are arranged as

A

SHELLS (Energy Level) (n) ->

SUBSHELLS (Sublevels) (l) ->

ORBITALS (Orientation) (m,)

46
Q

RULES GOVERNING FILLING ORDER

A
  1. Aufbau Principle
  2. Pauli’s Exclusion Principle
  3. Hund’s Rule
47
Q
  • Building-up principle
  • an electron occupies/fills the orbital with the lowest energy first.
A

AUFBAU PRINCIPLE

48
Q
  • No two electrons in the same atom can have the same set of four quantum numbers.
  • Paired electrons have opposite spins: allows two electrons with opposite spins to occupy the same orbital.
A

PAULI’S EXCLUSION PRINCIPLE

49
Q
  • Orbitals of equal energy are filled with one electron each before any one orbital is filled with a second electron.
  • Spins for single occupied orbitals must be the same (parallel).
A

HUND’S RULE

50
Q

Atoms must achieve a more stable electronic configuration like noble gases.

A

OCTET RULE

51
Q

outermost electrons

A

Valence electrons

52
Q

Atoms ________ so that cation has a noble-gas outer electron configuration.

A

lose electrons

53
Q

Atoms __________ so that anion has a noble-gas outer electron configuration.

A

gain electrons

54
Q

When a cation is formed from an atom of a transition metal, __________ are always removed first from the ns orbital and then from the (n – 1)d orbitals.

A

electrons

PIC LEC (5 decks)

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