CHEM Electron Configuration

अब Quizwiz के साथ अपने होमवर्क और परीक्षाओं को एस करें!

Pauli Exclusion Principle

maximum of two electrons may occupy an atomic orbital, but only if they have opposite spins

Full Configuration for Mg

1s²2s²2p⁶3s²

Electron Configuration for Si

1s²2s²2p⁶3s²3p²

Electron Configuration for Ar

1s²2s²2p⁶3s²3p⁶

Electron Configuration for Kr

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶

Electron Configuration for Sr

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²

Full Configuration for Rh

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d⁷

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p²

Ge

1s¹

H

1s²

He

Wavelength

Horizontal distance between two consecutive crests or troughs in a wave

Frequency

How many waves can pass a given point per second.

1s²2s²2p³

N

energy levels

what do the coefficients stand for? (1s²)

sublevels (or orbitals)

what do the letter symbols stand for? (1s²)

PAULI EXCLUSION PRINCIPLE

* 2 arrows in same box have to point in opposite ways * 2 electrons in same orbital have to spin in opposite ways

ORBITAL

* Always hold up to 2 electrons * Little boxes in orbital notation

HUNDS RULE

* Fill in each box once, then start filling in the second one * Bus rule

EXCITED STATE

* Higher energy (think of when did the flame test lab and the element changed color)

AUFBAU PRINCIPLE

* Last set of boxes might not be full... fill in order

GROUND STATE

* Lowest electron energy

SHORTHAND NOTATION

* Put the closest noble gas symbol in parenthesis * Continue electron configuration where it leaves off after noble gas

SUBLEVEL

* S sublevel- up to 2 electrons (I box) * P sublevels- up to 6 electrons (3 box) * D sublevels- hold up to 10 electrons (5 box) * F sublevels- hold up to 14 electrons (7 box) * Tell of the shape of the orbitals in each energy level

ORBITAL NOTATION

* Show electron configurations in more detail * Electrons in their orbitals * Each box represents one orbital and shows how many electrons (up to 2) are in that orbital * Little boxes under the sublevel

ENERGY LEVEL

* Where electrons are found * (2-8-8) * Big numbers represent the energy levels

# of orbitals in any s sublevel

1

# of orbitals in any p sublevel

3

p orbitals

3 mutually perpendicular dumbbell shaped orbitals; second to fill from 2nd energy level on up; can hold max of 6 electrons

# of orbitals in any d sublevel

5

d orbitals

5 orbitals of cloverleaf shape; third to fill for any energy level; beginning in the third shell, contains a total of 10 electrons; higher in energy than s and p orbitals in the same shell.

# of orbitals in any f sublevel

7

Photon

A quantum, or discrete amount, of light energy.

Atomic emission spectrum

A set of frequencies of electromagnetic waves given off by atoms of an element; consisting of a series of fine lines of individual colors.

Ground state

A state in which all the electrons in an atom have the lowest possible energies

Orbital

A three-dimensional region around the nucleus that indicates the probable location of an electron

1s²2s²2p⁶3s²3p¹

Al

1s²2s²2p⁶3s²3p⁶

Ar

Electron configuration

Arrangement of electrons in the orbitals of an atom.

Spectrum

Array of electromagnetic radiation displayed in order of wavelength

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p³

As

1s²2s²2p¹

B

1s²2s²

Be

Why do we fill the 4s orbital before the 3d orbital?

Because the 4s is lower in energy than the 3d, so it is filled first.

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁵

Br

1s²2s²2p²

C

1s²2s²2p⁶3s²3p⁶4s²

Ca

1s²2s²2p⁶3s²3p⁵

Cl

1s²2s²2p⁶3s²3p⁶4s²3d⁷

Co

1s²2s²2p⁶3s²3p⁶4s¹3d⁵

Cr

1s²2s²2p⁶3s²3p⁶4s¹3d¹⁰

Cu

Aufbau principle**

Electrons fill an atom in order of increasing energy level, starting at the lowest level.

1s²2s²2p⁵

F

1s²2s²2p⁶3s²3p⁶4s²3d⁶

Fe

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p¹

Ga

what happens to an electron when it absorbs energy?

Jumps to excited state

1s²2s²2p⁶3s²3p⁶4s¹

K

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶

Kr

1s²2s¹

Li

1s²2s²2p⁶3s²

Mg

1s²2s²2p⁶3s²3p⁶4s²3d⁵

Mn

1s²2s²2p⁶3s¹

Na

1s²2s²2p⁶

Ne

1s²2s²2p⁶3s²3p⁶4s²3d⁸

Ni

Pauli's exclusion principle**

No more than two electrons of opposite spin can occupy a given orbital.

1s²2s²2p⁴

O

Hund's rule**

Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin

1s²2s²2p⁶3s²3p³

P

1s²2s²2p⁶3s²3p⁴

S

1s²2s²2p⁶3s²3p⁶4s²3d¹

Sc

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁴

Se

1s²2s²2p⁶3s²3p²

Si

quanta

Small specific amounts of energy; The amount of energy needed for an electron to jump from one energy level to the next

Quantum

The amount of energy needed to move an electron from one energy level to another

1s²2s²2p⁶3s²3p⁶4s²3d²

Ti

1s²2s²2p⁶3s²3p⁶4s²3d³

V

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

Zn

Electromagnetic radiation

a form of energy that exhibits wavelike behavior as it travels through space

photons

a quantum of light; a discrete bundle of electromagnetic energy that interacts with matter similarly to particles

electron cloud

a region around the nucleus of an atom where electrons are likely to be found (most probable location)

Energy level

a region of set energy around the nucleus where electrons are likely to be found moving.

excited state

an electron in a temporarily higher energy level than in its ground state

valence electrons

an electron in the highest occupied energy level of an atom;available to be lost, gained, or shared in the formation of chemical compounds

How do you determine the # of Valence electrons?

by counting the # of s and p electrons since the most recent noble gas

Hund's Rule

electrons occupy equal energy orbitals so as to maximize the number of unpaired electrons

what happens to an electron when it releases energy?

falls to ground state

Erwin Schroedinger

he gave rise to the Quantum Mechanical Model with his calculation of the probability of where an electron can be found around the atom

Nitrogen

name the element 1s²2s²2p³

Aluminum

name the element 1s²2s²2p⁶3s²3p¹

Titanium

name the element [Ar]4s²3d²

Tungsten

name the element [Xe]6s²4f¹⁴5d⁴

orbitals

regions within electron cloud where electrons orbit the nucleus; number of orbitals differs with sublevel type (s,p,d,f)

sublevels

regions within the energy levels; corresponds to the block grouping s,p,d,f on the Periodic Table

s orbitals

spherical orbitals; first to fill for any energy level; can only hold 2 electrons

Aufbau Principle

states that each electron occupies the lowest energy orbital available

electron configuration

the arrangement of electrons in the energy levels, sublevels and orbitals of atoms

Hertz (Hz)

the unit of frequency, equal to one cycle per second

f orbitals

their shapes are even more complex than s, p, or d orbitals; can hold a total of 14 electrons in 7 sub-shells; in the fourth and fifth energy levels

shorthand notation

uses noble gas configuration from the preceding full level (stable core), along with electrons on current level

The number of electrons in a sublevel

what to the superscripts stand for? (1s²)

ground state

when all the electrons in an atom have the lowest possible energies


संबंधित स्टडी सेट्स

Critical Reading + Writing Written Assignment

View Set

Taylor: Fundamentals of Nursing, Ninth Edition - Chapter one quiz

View Set

Illinois Statutes and Regulations Pertinent to Accident & Health Only

View Set