Periodic Table
Energy required to remove an e- (electron).
Ionization Energy
These particles determine the mass number of an atom.
Protons and neutrons
What is an Ionic, Covalent, and Metallic bond?
Ionic: e- transfer metal to nonmetal.
Covalent: nonmetals share e- pairs.
Metallic: "sea of delocalized e-" shared among metal atoms.
This decay releases a helium nucleus.
Alpha decay
What is the molar mass of NaOH?
39.997 g/mol
Rounded: 40.00 g/mol
ADD THE ATOMIC MASSES OF EACH ELEMENT!!
Which has a larger atomic radius: K or Na? Explain.
K - located in period 4 and Na is in period 3.
Moving down a group you add another energy shell level moving Ve- further from the nucleus; resulting in a larger atomic size.
Explain why isotopes have different masses but similar chemical behavior.
Isotopes differ in number of neutrons but have the same number of protons and electrons
The geometry of NH₃ according to VSEPR theory.
Trigonal pyramidal
What is a naturally occurring radioactive element most commonly used for modern nuclear power plants?
Uranium
List in order of increasing electronegativity and EXPLAIN your reasoning.
As (Arsenic) Xe (Xenon) Br(Bromine)
Xe < As < Br
Noble gases = stable!!Compare alkali metals and alkaline earth metals in terms of valence electrons and ion charge.
Alkali metals (Group 1) - one valence electron and form +1 ions by losing that electron to achieve a stable configuration.
Alkaline earth metals (Group 2) have two valence electrons and form +2 ions by losing both, making them generally less reactive and harder than alkali metals.
How many protons, neutrons, and electrons are in an isotope of iron that has an atomic mass number of 54?
26 Protons
28 Neutrons
26 Electrons
What are intermolecular and intramolecular forces?
Intra - Stronger within atoms
Inter - Weaker between atoms
Bonus: Intra and Inter bond types.Name one medical and one energy application of nuclear chemistry.
Radiation therapy, Diagnostic imaging, Sterilization, etc.
Nuclear power plants
What's the weighted average?
Copper-63 62.93 amu 69.15%
Copper-65 64.93 amu 30.85%
63.55 amu
(0.6915 * 62.93) + (0.3085 * 64.93)
Why do elements in the same group show similar chemical properties?
Possession of the same number of valence electrons.
Valence electrons dictate how an element bonds, reacts, and interacts with other elements.
An element has 80% at 35 amu and 20% at 37 amu. Calculate.
35.4 amu
Bonus: What element would represent this?Oxygen (O) and hydrogen (H) form a polar covalent bond because…
Oxygen is more electronegative and pulls shared electrons closer
Compare nuclear fission and fusion.
Fission - Heavy atomic nuclei is split and less energy is released.
Fusion - Light atomic nuclei is collided and more energy is released.
What is the electron configuration for Sr (Strontium)?
1s22s22p63s23p63d104s24p65s2
Bonus: What's the noble gas configuration?
Element X has the following properties:
Period 3 and forms a 2− ion
Has a higher electronegativity than nitrogen
Has lower ionization energy than chlorine
Sulfur
EN higher than nitrogen (has one more electron than N) & Lower IE than chlorine (V electrons held less tightly)
An atom has 17 protons and 18 electrons. What element would this be?
1– charged ion (Cl⁻)
The molecular geometry of CH4 (methane) is ________, and the molecular geometry of CO2 (carbon dioxide) is ________.
Tetrahedral
Linear
When an element emits a gamma ray what happens to the atomic number and atomic mass?
The atomic mass and number remain the same.
Bonus: Explain what happens in Alpha and Beta.
Reactive metals from Group 1 and Group 2 often form compounds with nonmetals from Group 17.
Name the type of bond that is commonly formed between these atoms. Why do these groups tend to form this type of bond?
Groups 1 & 2 readily give up their valence electrons to become stable and atoms from Group 17 readily take on valence electrons creating an ionic bond.