Periodic Trends
When does atomic radius decrease?
What is going from left to right on the periodic table?
name of H₂SO₄
What is Sulfuric acid?
The group of metals that react with water.
What is Alkali Metals?
What type of bond involves the transfer of electrons?
Ionic Bond
Provide examples of one polar and nonpolar molecules.
H2O - polar
CH4 - non polar
The element has the highest electronegativity.
What is Fluorine?
The name of P₂O₅
What is Diphosphorus pentoxide?
Name 3 metalloids
What is Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, Polonium, and Tennessine?
Definition of polar bond
A covalent bond where electrons are unequally shared.
What is the formula for formal charge?
Formal Charge= Valence Electrons − (Non-bonding Electrons + 1/2 × Bonding Electrons)
The reason for noble gases not having electronegativity.
They have a full valence shell and don't need to attract electrons.
Name the acid HClO₃
What is Chloric acid?
The group on the periodic table with high reactivity, high electron affinities, and their melting and boiling points increase as you move down the group.
What is Halogens?
What difference does the electronegativities of two bonded atoms need to have for the bond to be polar?
Between 0.7 and 1.7.
How to determine neutrons for isotopes?
Subtract atomic number - mass number
Definition of electron affinity.
Electron affinity is defined as the change in energy of a neutral atom when an electron is added to the atom to form a negative ion. In other words, the neutral atom's likelihood of gaining an electron
The name of the compound with the formula MnO₂
What is Manganese(IV) oxide ?
The only metal that is a liquid at room temperature?
What is Mercury (Hg)?
Rank the following bonds from most polar to least polar:
C–O, N–H, F–F
N–H > C–O > F–F
Why do metals conduct electricity while most covalent compounds do not?
Metals have a "sea of delocalized electrons", meaning their valence electrons are free to move, allowing them to conduct electricity.
Covalent compounds have localized electrons in bonds and do not have free-moving charged particles.
Put the following species in order from smallest to largest atomic/ionic radius:
Si, P, K, Ca²⁺, Br⁻
Ca²⁺ < Si < P < Br⁻ < K
Name CuSO₄·5H₂O
What is Copper(II) sulfate pentahydrate?
What does the period number tell you about an element?
The number of energy levels (electron shells) it has.
What is the significance of the octet rule in chemical bonding? Are there any exceptions to this rule?
The octet rule is a fundamental concept in chemistry that states atoms tend to form bonds in such a way that each atom has eight electrons in its valence shell, achieving a stable electron configuration similar to that of noble gases.
Some elements are stable with fewer than eight electrons in their valence shell. Example is beryllium (4 electrons)
Elements in the third period and beyond can have more than eight electrons in their valence shell due to the availability of d-orbitals. Example is phosphorus (up to 10 electrons)
What element has the smallest atomic radius?
Helium