Atom structure (P.E.N.)
Electron Configuration (Orbitals)
Bonding Basics
Bondings part 2
100
What subatomic particle is positively charged and found in the nucleus?
Proton
100
What is the name of the first and most spherical electron orbital?
s-orbital.
100
What type of bond forms when oppositely charged ions attract each other?
Ionic Bond
100
What type of bond involves a central metal atom surrounded by ligands containing lone pairs of electrons?
Coordination Bond
200
Besides protons, what other particle lives in the nucleus?
Neutron
200
P orbitals have a dumbbell shape. How many p orbitals are present in a given energy level?
Three
200
Ionic compounds typically have high melting and boiling points. Why?
Strong electrostatic attraction between oppositely charged ions
200
Diamond is a giant covalent structure, resulting in its extreme hardness. Why does this structure make diamond so hard?
The strong covalent network throughout the entire structure makes it difficult to break bonds.
300
What scientist experimented with cathode rays, leading to the discovery of the electron?
J.J. Thomson
300
When writing electron configurations, we use a small number next to a letter. What does this number tell us?
It tells us how many electrons are in that specific area.
300
What subatomic particle is formed when an atom gains or loses electrons?
Ion
300
Metallic bonding involves a "sea" of delocalized electrons. How does this "sea" contribute to the electrical conductivity of metals?
The delocalized electrons are free to move throughout the metal, allowing them to carry current.
400
Imagine an atom like a solar system. Electrons travel around the nucleus in specific paths. What is the name for these paths?
Electron orbitals
400
Explain why some elements, like copper (Cu) and chromium (Cr), have exceptions to the typical electron configuration order.
Copper (Cu) and chromium (Cr) exhibit exceptions to the Aufbau principle due to increased stability achieved by an irregular electron configuration.
400
In covalent bonding, atoms share electrons. How does electronegativity affect the polarity of a covalent molecule?
A higher difference in electronegativity creates a polar molecule with a partially negative and positive end.
400
Intermolecular forces are weaker attractions between molecules compared to the forces within a molecule. Explain the difference between London dispersion forces and dipole-dipole interactions.
London dispersion forces are weak, temporary attractions between all molecules, while dipole-dipole interactions are stronger attractions between polar molecules due to their positive and negative ends.
500
Atoms of the same element can have different numbers of neutrons. What is the name for these variations of an element?
Isotopes
500
Write the complete electron configuration for the element magnesium (Mg) with atomic number 12
1s²2s²2p⁶
500
Draw the Lewis structure for water (H2O) showing the shared electrons and lone pairs.
500
Hydrogen bonding is a particularly strong intermolecular force due to the high electronegativity of hydrogen. How does hydrogen bonding influence the properties of water (H2O)?
Hydrogen bonding allows water molecules to form a network, influencing water's properties like high boiling point and surface tension.