Adv Chemistry - Midterm

Dalton

Developed a modern atomic theory but was unaware of subatomic particles

Rutherford

Found the nucleus stating that it is very small, positively charged, and dense

Mendeleev

Father of periodic table (1869)

JJ Thomson

Stated that electrons are like raisins in plum pudding (+ and – mixed together)

Schrödinger

Modeled electrons as waves

Bohr

Planetary model of atom (1913)

Moseley

Arranged the periodic table by atomic number

Atom

The smallest particle of an element that retains the properties of that element.  

Isotopes

Atoms with the same # of protons, but different # of neutrons in the nucleus of an atom.  

Mass Number

The total number of protons and neutrons in the nucleus of an atom.

Electron

A negatively charged subatomic particle  

Atomic Number

The number of protons in the nucleus of an element.

Neutron

A subatomic particle with no charge.  

Proton

A positively charged subatomic particle  

Average Atomic Mass

The weighted average of the masses of the isotopes of an element. Found on the periodic table; measured in AMU

Correctly list the following atoms in order of increasing atomic radius (smallest to largest). S, Ar, P, Mg

Ar, S, P, Mg

Correctly list the following atoms in order of increasing atomic radius (smallest to largest). Ca, Ba, Mg, Be  

Be, Mg, Ca, Ba

Why is a cation smaller than the original neutral atom?  

It loses its valence energy level when it loses electrons, shrinking the radius significantly.

Why is an anion larger than the original neutral atom?  

It gains electrons to fill its valence shell, which expands the cloud slightly

Correctly list the following groups in order of increasing electronegativity (lowest to highest).  Alkali metals, halogens, transition metals, alkaline earth metals. 

Alkali Metals, Alkaline Earth Metals, Transition Metals, Halogens

Correctly list the following atoms in order of increasing electronegativity (lowest to highest): Br, I, F, Cl 

I, Br, Cl, F

Why do noble gases not have electronegativity values?  

No attraction for electrons bc full valence shell

Correctly list the following elements in order of decreasing ionization energy (highest to lowest):  N, Ba, Be, He

He, N, Be, Ba

1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², 4f⁵

Inner transition metal

1s², 2s², 2p⁶, 3s² 

Alkaline earth metal

 1s², 2s², 2p⁶, 3s², 3p⁶ 

Noble Gas

 1s², 2s², 2p⁶, 3s², 3p⁵ 

Halogen

1s², 2s², 2p⁶, 3s¹ 

Alkali metal

 1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d⁵

Transition metal

Why did Mendeleev leave blanks in his periodic table?  

He predicted the existence of other elements yet to be discovered.  Patterns in properties of elements and average atomic masses suggested they should exist.

How did Moseley change Mendeleev’s periodic table? 

He re-organized the periodic table by atomic number (vs. average atomic mass from Mendeleev)

List the types of electromagnetic radiation in order of highest frequency to lowest frequency. Microwaves, X-ray, visible light, infrared, ultraviolet, gamma radiation, radio

Gamma, X-Ray, UV, Visible, IR, Microwave, Radio

Alkali metals

Soft, shiny, solid, highly reactive, low electronegativities

Alkaline earth metals

Malleable, conductive, solid

Halogens

Gasses, liquid, and solid, highly reactive nonmetals, high electronegativities

Noble Gasses

All gasses, most stable elements, 8 valence electrons 

Ionic Bond Characteristics

Crystal lattice

>=1.7EN

High melting/boiling point

Soluble

M/NM

Electrolyte, conductive

Electrons transferred

Covalent Bond Characteristics

Linear, bent, trigonal planar, trigonal bi-pyramidal, tetrahedral, octahedral

0-1.69EN

Low melting/boiling point

Insoluble (UNLESS acid, sugar, organic)

NM/NM

Nonelectrolye (UNLESS acid)

Electrons shared

Metallic Bond Characteristics

<1 EN

High melting/boiling point

Insoluble

M/M

Nonelectrolyte, conductive

Sea of electrons

Arrange IMFs from strongest to weakest: London Dispersion Forces, Hydrogen Bonding, Ionic, Dipole-Dipole

Ionic, Hydrogen Bonding, Dipole-Dipole, London Dispersion Forces

Compounds that contain what element are considered organic? 

Carbon

How can you tell the difference between alkane, alkene, and alkyne hydrocarbons?

Alkanes contain only single bonds.  Alkenes contain at least 1 double bond and no triple bonds.  Alkynes contain at least 1 triple bond.

What is the difference between methane, ethane, propane, and butane?

Number of carbons in the chain.  Meth = 1, Eth = 2, Prop = 3, and But = 4

What to do to increase rate of dissolving (increase or decrease) for a SOLID SOLUTE?

Temperature:

Stirring:

Surface Area:

Temperature: Increase

Stirring: Increase

Surface Area: Increase

What to do to increase rate of dissolving (increase or decrease) for a GAS SOLUTE?

Temperature:

Stirring:

Pressure:

Temperature: Decrease

Stirring: Decrease

Pressure: Increase

Which factor changes the solubility of a compound?

Temperature

How is heat different from temperature?

Heat is energy transferred between two objects based upon a difference in their temperature. Temperature is a measure of average kinetic energy.

What is specific heat? 

The amount of heat required per gram to raise the temperature of a substance by 1℃.
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