Question

fill-in with the best word or phrase.

1. an electron has lower potential energy when it is _______________ to the nucleus.
2. p sublevel has ____ orbitals and holds a max of ____ electrons.
3. atoms (and electrons) are most stable in their _____________ _____________ energy state.
4. all atoms have their 1st electron fill in what n and sublevel? ______
5. the order of increasing principal energy levels is from ____ to ____.
6. _________________ principle states that there is a max of __ electrons in a single orbital and that they must have _________________ spin.
7. the ______________ principle states that electrons fill an electron configuration for a ground state atom from __ energy to ____ energy
8. the name of the current atomic model is the _________________ _________________ model.
9. all noble gasses have ______ valence electrons.
10. given the symbol 3s², the 3 is the ____________________________ the s is the ___________ and the 2 is the ____________________________
11. valence electrons determine the ____________________________ properties of an element including ___________ and _____________
12. a row on the periodic table is called a ___________________
13. a column on the periodic table is called a _________________ or _________________
14. the sublevel defines the ______ of the probability electron density cloud.
15. the outermost occupied principal energy level is the _________________ shell and holds a maximum of __ electrons (except for he, which has __ outermost electrons). this is also called a complete _____________.
16. an electron has a dual nature; it can behave as both a _____________ and a ____.

Explanation:

These questions are about atomic structure and electron behavior, which falls under Chemistry (a subfield of Natural Science). Let's answer each:

1. An electron has lower potential energy when it is closer to the nucleus (electrostatic attraction; closer = lower PE).
2. P sublevel has 3 orbitals (pₓ, pᵧ, pz) and holds a max of 6 electrons (2 per orbital × 3).
3. Atoms (and electrons) are most stable in their lowest (or ground) energy state (minimum energy = stability).
4. All atoms have their 1st electron fill in n=1, s (1s orbital, lowest energy).
5. The order of increasing principal energy levels is from lower to higher (n=1 < n=2 < ...).
6. Pauli Exclusion Principle: max 2 electrons per orbital, with opposite spin.
7. Aufbau Principle: electrons fill from lowest to highest energy (build-up order).
8. Current atomic model: Quantum Mechanical model (describes electron probability clouds).
9. All noble gases (except He) have 8 valence electrons (He has 2; full outer shell).
10. In \( 3s^2 \): 3 = principal quantum number (n) (energy level), s = sublevel, 2 = number of electrons.
11. Valence electrons determine chemical properties (e.g., reactivity, bonding) like reactivity and bonding behavior.
12. A row on the periodic table is a period.
13. A column is a group (or family).
14. Sublevel defines the shape of the electron density cloud (s=spherical, p=dumbbell, etc.).
15. Outermost occupied level: valence shell; max 8 electrons (He: 2); complete octet (or duplet for He).
16. Electron dual nature: particle and wave (wave-particle duality).

Answer:

1. closer
2. 3; 6
3. lowest; energy
4. n=1, s
5. lower; higher
6. Pauli Exclusion; 2; opposite
7. Aufbau; lowest; highest
8. Quantum Mechanical
9. 8 (He: 2)
10. principal quantum number (n); sublevel; number of electrons
11. chemical; reactivity; bonding (or similar properties)
12. period
13. group; family
14. shape
15. valence; 8; 2; octet (duplet for He)
16. particle; wave