Chemistry Gr 12 Unit 1

radio, microwave, infrared, visible, UV, X-ray, gamma ray

How often. Measured in Hz or S^-1

Colour. Measured in distance (usually nm)

“intensity”, “brightness”, “loudness”, “height”

ROYGBIV

Energy goes up

1x10^-9

metre, milli (-3), micro (-6), nano (-9), pico (-12)

It should have emitted white light bc electrons can absorb all wavelenths of energy so they should’ve radiated off all as well.

In the end the hydrogen emitted a pink light. When the light was shown through a prism instead of there being all the colours, there were only a specific colours of red, green, blue and violet. This demonstrated that only specific wavelengths could be absorbed by the Hydrogen atom. (staircase model)

656nm (red, 3 → 2), 486nm (green, 4 → 2), 434nm (blue, 5 → 2), 410nm (violet, 6 → 2)

The specific wavelengths that are produced when an electron falls from one ring to another. It has black spaces and coloured lines.

The colours absorbed by the element. This is seen as the opposite of the emission spectrum as the specific quantities that release a specific light can’t be on the absorbtion spectrum as it would move the elctron onto the next ring. The absorbtion spectrum has black lines and coloured spaces.

Calculation of when electrons fall to the first ring. Produces UV light.

calculation of when electrons fall to the second ring

Calculation of when electrons fall to the third ring. Produced infrared results

The Aufbau principle states that electrons fill the lowest energy levels first before moving to higher energy levels in an atom.

an orbital can have a max of 2 electrons and they must have opposite spins

Hund's rule states that when filling orbitals of equal energy, electrons will occupy separate orbitals

bottom to top

S orbitals have a spherical shape that gets bigger for every added number

8s, infinity, and rotated 8 getting progressively bigger for every added number

4 leaf clover, rotated 5 times and gets bigger for each number

a flower with 6 petals, rotated 7 times, bigger for each number

s+p of highest quantum number

1s2 2s2 2p6 3s2 3p6 4s2 3d10 …

[noble gas] 2s2 2p6 3s2 3p6 4s2 3d10 …

use previous noble gas and full config

[noble gas] horizontal lines

an ion with a negative charge bc it has gained an electron

an ion with a positive charge bc it has lost an electron

cross out the valence electrons that are removed

cross out the previous number and replace it with the added one

copper (Cu), silver (Ag), and Gold (Au)

one of the valence s electrons moves to d orbital to fill it in the ground state

Ferromagnetic refers to materials that have a strong attraction to magnetic fields, allowing them to become magnetized even when the magnetic field is removed.

Paramagnetic refers to a substance or material that is weakly attracted to a magnetic field due to the presence of unpaired electrons. These elements magnetism disappears when the field is removed

Diamagnetic is a property of materials that are not attracted to a magnetic field and have no permanent magnetic moment.

a “postal code” indicating the location or position of an electron

n, l, ml, ms

n (number of energy levels)

1 → infinite

L (orbital shape)

0 → n-1

ml (orbital orientation)

-L → +L

ms (electron spin)

-1/2 or +1/2

the positive/negative sign

Principal quantum number(n) and effective nuclear charge (Z_eff)

principal quantum number

it increases

it decreases

the distance between the nuclei of 2 adjacent atoms

atomic number (z) - shielding electrons (non valence electrons) (s)

Since the electrons repel each other, the resulting anion has a larger AR

the energy given off when an electron is added to an atom

the measure of the electron attracting ability of an atom

the energy required to remove an electron from an atom

IE decreases

IE increases

B, Al, O, S

The ionization energy decreases from Be to B and Mg to Al due to the shielding effect. The shielding effect occurs when inner electrons (1s, 2s namely) shield the outermost electron from the full positive charge of the nucleus, reducing the ionization energy. Therefore, the ionization energy decreases.

The ionization energy is reduced due to the repulsion between the paired electrons in the 2p/3p, making the electron easier to remove.

isoelectronic

the n value / principal quantum number

the orbital type (l) (s,p,d,f)

a specific region where a max of 2 electrons can be found

The forces of attraction between molecules, determining their physical properties. Examples include hydrogen bonding, dipole-dipole interactions, and London dispersion forces.

Forces that hold atoms together within a molecule. They include covalent bonds, which involve the sharing of electrons, and ionic bonds, which involve the transfer of electrons between atoms. These forces determine the structure and properties of a molecule.

it means that the compound is more ionic

It means the compound is more covalent

Chemical bonds formed between atoms by the transfer of electrons. They occur between a metal and a non-metal, resulting in the formation of ions with opposite charges.

A 3D arrangement of positive and negative ions held together by electrostatic forces. It forms repeating unit cells, creating a stable structure.

anions

The energy required to break apart one mole of an ionic solid into its constituent ions in the gas phase. It measures the strength of the ionic bond in the solid.

Primary: high charge and low AR

Secondary: high boiling point, high melting point, conduct electricity in (aq), (g), (l) states

it is pure covalent

valence electrons (VE) - non bonding electron (NB) - Bonds

No, while CNOF tends to follow it, as you move down the periodic table, it becomes more likely.

A coordinate covalent bond is a type of chemical bond that is formed when both electrons in the shared pair come from the same atom

when the central element in an atom has a valence shell greater than 8

when the central element in an atom has a valence shell less than 8

Need:

1. calculate the needed electrons

   Have:

2. calculate the number of electrons the elements already have

3. add/subtract the charge

   For bonds:

4. Need-Have

   For electrons:

5. Have - Bonds(2)

   Drawing:

6. Lowest electronegative element in the middle

7. draw bonds

8. place electrons going from outside to inside

9. put square brackets and charge

No

when a double bond can be drawn with the double bond in 2+ locations without changing the arrangement of the atoms.

Resonance hybrids are multiple Lewis structures that represent a molecule's real structure. They are formed when a molecule can be represented by more than one valid Lewis structure.

the arrows showing the movement of the double bonds

they are delocalized

it means they are shared over all the bonds

the distribution of charge on the entire molecule

many physical and chemical properties such as it’s state

A physical property is a characteristic of matter that is not associated with a change in its chemical composition. Familiar examples of physical properties include density, color, hardness, melting and boiling points, and electrical conductivity.

A chemical property is any of a material's properties that becomes evident during, or after, a chemical reaction

Examples of chemical properties include flammability, toxicity, acidity, reactivity

1. check bond polarity

2. use the shape to see the symmetry of polarity

3. note the effect of lone electron pairs on the central atom

4. indicate direction of polarity using arrow pointing to the more electronegative end

Hydrogen bonding is a type of intermolecular force that occurs when a hydrogen atom, covalently bonded to a highly electronegative atom such as oxygen, nitrogen, or fluorine, is attracted to another electronegative atom in a different molecule. This attraction results in a relatively strong bond between the molecules.

Dipole-dipole bonding is a type of intermolecular force that occurs between polar molecules. It results from the attraction between the positive end (or pole) of one molecule, which has a partial positive charge, and the negative end (or pole) of another molecule, which has a partial negative charge

Ion-dipole bonding is a type of chemical interaction between an ion (charged particle) and a polar molecule. It occurs when the positive or negative charge of the ion attracts the partial charges of the polar molecule.

Ion-induced dipole bonding is a type of intermolecular interaction that occurs when a charged ion induces a temporary dipole moment in a nearby neutral molecule or atom.

Dipole-induced dipole bonding occurs when a polar molecule induces a temporary charge on another molecule. For example, the negative side of an HCl molecule will repel the negative electrons of O2 creating temporary positive and negative sides.