Metallic Properties

Metallic Properties:

Metals are sometimes described as a lattice of positive ions surrounded by a cloud of delocalized electrons. They are one of the three groups of elements as distinguished by their ionization and bonding properties, along with the metalloids and nonmetals. On the periodic table, a diagonal line drawn from boron (B) to polonium (Po) separates the metals from the nonmetals. Most elements on this line are metalloids, sometimes called semi-metals; elements to the lower left are metals; elements to the upper right are nonmetals (see the periodic table showing the metals).

Source: http://wiki.answers.com/Q/Metallic_and_non_metallic_propertyhttp://wiki.answers.com/Q/Metallic_and_non_metallic_property

Atomic radius

The atomic radius of a chemical element is a measure of the size of its atoms, usually the mean or typical distance from the nucleus to the boundary of the surrounding cloud of electrons. Since the boundary is not a well-defined physical entity, there are various non-equivalent definitions of atomic radius

Source: http://en.wikipedia.org/wiki/Atomic_radius

Video:

Atomic radius: http://www.youtube.com/watch?v=fBazliON32I

Metallic properties: http://www.youtube.com/watch?v=ZwTmKApE2Jg

Ionic and Covalent Bonding

IONIC BONDING
An ionic bond is a chemical bond formed by the electron attraction between positive and negative ions


COVALENT BONDING

Covalent Bonds are chemical bonds formed by the sharing of a pair of electrons between atoms


Examples:

Ionic Bond: NaCl

Total Number of Electrons: 8


There are no extra electrons so the drawing is done.

Covalent Bond: HCl

Total Number of electrons : 8

Covalent Bond: FCl₄⁺

GROUPS

- Elements in a group have the same valence electrons.

FAMILIES

IA - Alkali metals

IIA - Alkali earth metals

IIIA - Boron

IVA - Carbon

VA - Nitrogen

VIA - Chalcogens

VII - Halogens

VIII - Noble gas / Ideal gas

Scientific Measurements

Measurements

- the process of estimating or determining the magnitude of a quantity, such as length or mass, relative to a unit of measurement, such as metre or kilogram.

Units of Measurements

- Definite magnitude of a physical quantity, defined and adopted by convention and/or by law that is used as a standard for measurement of the same physical quantity.

SI BASE UNIT

1) Meter for length 

2) Kilogram for mass 

3) Second for time 

4) Kelvin for temperature 

Calibration

- Comparison between measurements - one of known magnitude or correctness made or set with one device and another measurement made in as similar a way as possible with a second device.

Accuracy

  - The degree of closeness of measurements

- Correctness, Exactitude, Exactness, truth

Precision

- The state or quality of being precise; exactness.

Place Values

 for whole numbers:

PRACTICE HERE: http://www.aaamath.com/plc41ax3.htm

for decimals:

 PRACTICE HERE: http://www.aaamath.com/plc51bx2.htm#pgtp

Quantum Numbers

Quantum Numbers

In quantum numbers always use the last electron
configuration in knowing the element`s “n, l, mL, mS”
♥ n- principal quantum
♥ l- azimuthal quantum
♥ mL- magnetic quantum
♥ms- magnetic spin quantum
For example:
6C : 1s2 2s2 2p6
12

Note: We'll be using Carbon as our example

♥ n- describes the energy level, an electron is located in.

Example: 2p6
               n= 2

♥ l- Sublevels in the atoms of the knownelements are s- p- d - f .
♥ describes the shape of the orbital.

Example: 2p6
               l= 1

Why 1?, because in the chart it shows that if the sublevel is p its 1.
















♥ mL-describes the orientation in space for the orbital.

Example: 2p6
               mL- 0

Take Note!!

♥ mS- Describes the spin of an electron.

Example: 2p6
               l= +1/2

Why +1/2?, because if the last arrow Is arrow down its –1/2 because it is
spinning counterclockwise, if its arrow up its +1/2 because it spins clockwise.

Electron Distribution

Electron distribution mnemonics


-The orbital names s, p, d, and f stand for names given to groups of lines in the spectra(plural of spectrum-The distribution of energy, arranged in order of wavelengths). These line groups are called sharp, principal, diffuse, and fundamental.

-A function which gives the number of electrons per unit volume of phase space.
Electron Configuration

-arrangement of electrons of an atom, a molecule, or other physical structure. It concerns the way electrons can be distributed in the orbitals of the given system (atomic or molecular for instance).

Energy levels

-An atom consists of electrons orbiting around a nucleus. However,the electrons cannot choose any orbit they wish. They are restricted to orbits with only certain energies. Electrons can jump from one energy level to another, but they can never have orbits with energies other than the allowed energy levels.



-can only take on certain discrete values of energy, as opposed to classical particles, which can have any energy.



Bigger orbit =higher energy



Energy levels are said to be degenerate, if the same energy level is shared by more than one quantum mechanical state. They are then called degenerate energy levels.

Videos

Energy level

http://www.youtube.com/watch?v=Y9HgalWNCbI



Shell

-The main energy level in which an electron resides. It is given by the principle quantum no. , which is denoted by “n”. “n” can have a positive integral (quantized).

Subshell

-This is the sub-energy level in which the electron resides. It is given by the azimuthal quantum number, denoted by “L”, satisfies the inequality.



Orbital

This is an orientation a subshell takes up in presence of an external magnetic field. It is given by the magnetic quantum number “m”.


Electron distribution mnemonics


-The orbital names s, p, d, and f stand for names given to groups of lines in the spectra(plural of spectrum-The distribution of energy, arranged in order of wavelengths). These line groups are called sharp, principal, diffuse, and fundamental.

-A function which gives the number of electrons per unit volume of phase space.





Electron Configuration

-arrangement of electrons of an atom, a molecule, or other physical structure. It concerns the way electrons can be distributed in the orbitals of the given system (atomic or molecular for instance).





Energy levels

-An atom consists of electrons orbiting around a nucleus. However,the electrons cannot choose any orbit they wish. They are restricted to orbits with only certain energies. Electrons can jump from one energy level to another, but they can never have orbits with energies other than the allowed energy levels.



-can only take on certain discrete values of energy, as opposed to classical particles, which can have any energy.



Bigger orbit =higher energy



Energy levels are said to be degenerate, if the same energy level is shared by more than one quantum mechanical state. They are then called degenerate energy levels.



Videos

Energy level

http://www.youtube.com/watch?v=Y9HgalWNCbI



Shell

-The main energy level in which an electron resides. It is given by the principle quantum no. , which is denoted by “n”. “n” can have a positive integral (quantized).



Subshell

-This is the sub-energy level in which the electron resides. It is given by the azimuthal quantum number, denoted by “L”, satisfies the inequality.


Subshell label L Max.electrons Shells containing it. Historical name

S 0 2 Every shell Sharp

P 1 6 2nd shell + Principle

D 2 10 3rd shell+ Diffuse

F 3 14 4th shell + Fundemental

Atoms

ATOMS

→ the smallest mediaeval unit of time, equal to fifteen ninety-fourths of a second.

→ a theoretical particle of matter, imagined to be incapable of further division; the smallest possible unit of substance.

Sub-atomic Particles:

Protons:

→ a positively charged subatomic particle forming part of the nucleus of an atom → determines the atomic number of an element.

Electron:

→ the subatomic particle having a negative charge

→ orbiting the nucleus; the flow of electrons in a conductor constitutes electricity.

Neutron:

→ subatomic particle forming part of the nucleus of an atom

→ no charge.

How to Determine the Atomic and Mass Number:

• Atomic Number

→ number of protons in the nucleus of an atom determines an element's atomic number

• Mass Number

→ determined by the number of protons and neutrons in an atom

Ex:

* Isotope - Any of two or more atoms of an element having the same number of protons, but a different number of neutrons in its nucleus. (same atomic number but not mass number)

Ex:

IONS

→ an atom or molecule in which the total number of electrons is not equal to the total number of protons, giving it a net positive or negative electrical charge

• Anion – gains electrons (negative)

Ex:

• Cation - loses electrons (positive)

Ex:

AZPEN*

Formula:

• A (mass number) = P + N

• Z (atomic number) = P

• P (proton) = Z

• E (electrons) = P - [charge of ion]

• N (neutron) = A - Z