Chemistry: Midterm Review

Fluorine

nucleus, 1 AMU, positive

nucleus, 1 AMU, neutral

electron cloud, 1/1836 AMU, negative

An isotope is a version of an element with a different number of neutrons. The atomic mass, and number are needed for isotope notation.

Nihonium

sulfur has 6 valence electrons, and so does oxygen.

-3

Alkalai metals

1s²2s² OR [He] 2s²

1s²2s²2p⁶3s²3p⁶ OR [Ne] 3s²3p⁶

D and F

silicon

zirconium

Malleable (ductile), lusterous, conducts heat/electricity.

Dull (not lusterous), brittle, poor conductor of heat/electricity?

Semi-conductive, brittle or malleable/ductile, sometimes lusterous

A photon is emitted.

Steps…

1. atom gains energy from outside source

2. energy causes atom to jump to excited state (higher energy orbital)

3. electrons eventually leave excited state and return to a ground state (starting orbital)

4. when electrons go back to a ground state, it emits a photon (energy exits) and its wavelength (related to energy) dtermines the color of the light seen

597 nm

Gases A, B, and D are in the compound. The lines of those gases match up to the unkown mixture.

Gamma rays have the highest, and radio waves have the lowest

Photons (only radiation humans can see)

-Wavelengths from 400nm to 750nm

Red: 750-620 Lowest Energy/Longest Wavelengths

Orange: 620-590

Yellow: 590-570

Green: 570-495

Blue: 495-450

Violet: 450-400 Highest Energy/Shortest Wavelength

a complete visible spectrum

colored photons emitted by a substance (unique for every atom/element)

opposite of emmision spectra

Wavelengths of the photon being emitted

increase

increase

decrease

Medeleev, organized by atomic mass

Mosley, organized by atomic number (protons in an element) and metals and nonemetals.

How pronounced metallic properties are in elements

How large the atom is (size not mass)

• distance from nucleus to outer-most orbital

The atom’s potential to attract (gain) electrons from other atoms (How badly it wants to)

• the larger the number to more potential

• how likely the atom is going to gain electrons

The energy required to remove an electron form an element (goes with electronegativity)

• getting rid of electrons

• for every electron lost - ionization energy increases (10 electrons = 10 energies)

• Every time you lose one, the next is harder to lose

• when there is a large increase the atom is done losing electrons

Shows where the electrons are in sub-orbitals if an atom (it is another layer to Bohr models)

1. Find the amount of valence electrons (don’t draw nucleus like a Bohr model)

2. Draw the chemical symbol

3. Pick 1 side first (NO CORNERS)

4. *remeber electrons hate pairing up unless it is needed (similar to seats on a bus). 4 spots (start top, go clockwise)

   KEY: DOTS=VALENCE ELECTRONS (8 max)

An atom that has gained a charge due to a change in the number of electrons.(result of ionic bonds/compounds)

A cation has a positive charge, it is the element losing valence electrons, and it is the metal in the ionic compound

AN anion has a negative charge, it is the element gaining valence electrons, and it is the nonmetal in the ioic compound.

The oxidation state.

metals →stay the same (normal)

nonmetals →change ending to -ide

Combination of metal and nonmetal properties (similar to metalloids)

1. Form crystals (rough shape) (ex. table salt)

2. Brittle

3. Soluble in water (dissolves)

4. Only conduct elecctricity when dissolved in water

5. High melting/boiling points

Yes, covalent compounds create molecules.

Multiple nonmetals (2+)

Overlapping valence shells.

• shared electrons (bonds)(complete valence shell)

• paired eletrons (don’t touch)

mono

di

tri

tetra

penta

hexa

septa

octa

deca

the more electronegative one

Valence Shell Electron Pair Repulsion

covalent bonds and lone pairs space out as much as possible around the central atom

• can be used to determine shape

Number of bonds + number of lone pairs

• same thing as electron group