Question

nucleus. can you describe 3 ways which (or three properties of) the relationship between the orbiting electrons and the positive nucleus change as you have atoms with more protons and electrons? what is effective nuclear charge, and what does that have to do with the 3 properties you identified? you may want to use section 6.5 for your answer. using this knowledge, can you solve the following problem? a. the noble gases are found in the last group, or most right - hand column of the periodic table. they are characterized as being inert, or not very likely to participate in a chemical reaction. using their values of electron affinity and ionization energy, can you explain why the noble gases tend not to participate in chemical reactions? b. the halides are the chemicals in the second most right - hand column, or group, of the periodic table. unlike the noble gases, these chemicals very often will participate in chemical reactions, specifically by borrowing electrons from their neighbor. using their values of electron affinity and ionization energy, can you explain why the halides like to obtain electrons from other chemicals or compounds? c. the alkali metals and alkali earth metals are the chemicals in the left - most and second left - most column, or group, of the periodic table. using their values of electron affinity and ionization energy, can you predict how these metals will participate in chemical reactions? will they borrow electrons or donate them to other chemicals or compounds? 5. drawings a. can you draw a 1s orbital and a 2s orbital, and label each? how many electrons can go into each orbital? which has more energy? b. can you draw a 2p orbital and a 3s orbital and label each? how many electrons can go into each orbital? which has more energy? c. can you draw a 3p and 3d orbital and label each? how many electrons can go into each orbital? which has more energy? d. can you draw 4d, 5p, and 6s orbitals and label each? how many electrons can go into each orbital? which has more energy? e. using the periodic table, can you tell for any element, what the highest energy orbital is? why is that information important? if electrons determine how an atom participates in chemical reactions, what does knowing what the highest energy orbital tell us? (hint, the periodic table was originally constructed based on how chemicals behaved in reactions, and yet somehow, it also easily shows an atoms electron configuration. why do you think that is?) the highest - energy orbital which is valence dictates reactivity. tells if an element donates, accepts, or shares electrons. the periodic table structure mirrors orbital filling.

Explanation:

Step1: Define effective nuclear charge

Effective nuclear charge ($Z_{eff}$) is the net positive charge experienced by an electron in a multi - electron atom. It is calculated as $Z_{eff}=Z - S$, where $Z$ is the atomic number (number of protons) and $S$ is the shielding constant.

Step2: Three properties of electron - nucleus relationship

1. **Atomic radius**: As the number of protons increases, the effective nuclear charge increases. This pulls the electrons closer to the nucleus, decreasing the atomic radius.
2. **Ionization energy**: Higher effective nuclear charge means more energy is required to remove an electron from the atom, so ionization energy increases.
3. **Electron affinity**: A higher effective nuclear charge makes the atom more likely to attract additional electrons, increasing electron affinity in general trends across a period.

Step3: Noble gases

Noble gases have a full outer - shell electron configuration. They have a relatively high ionization energy because removing an electron would disrupt this stable configuration. Their electron affinity is low or even positive in some cases because adding an electron would put it in a new, higher - energy shell. So, they tend not to participate in chemical reactions.

Step4: Halides

Halides have a high electron affinity because they need one more electron to achieve a stable noble - gas electron configuration. Their ionization energy is also relatively high but not as high as noble gases. They like to obtain electrons from other chemicals or compounds to complete their outer shell.

Step5: Alkali and alkaline - earth metals

Alkali metals and alkaline - earth metals have low ionization energies because they have one or two valence electrons that are easily removed to achieve a stable electron configuration. They have low electron affinities as well. So, they will donate electrons in chemical reactions.

Step6: Orbital drawings and properties

1s and 2s orbitals

- **Drawing**: A 1s orbital is a spherical shape centered around the nucleus. A 2s orbital is also spherical but larger in size than the 1s orbital.
- **Electron capacity**: Both 1s and 2s orbitals can hold 2 electrons.
- **Energy**: The 2s orbital has more energy than the 1s orbital because it is farther from the nucleus.

2p and 3s orbitals

- **Drawing**: A 2p orbital has a dumb - bell shape with three different orientations ($p_x$, $p_y$, $p_z$). A 3s orbital is spherical and larger than the 2s orbital.
- **Electron capacity**: A 2p orbital can hold 6 electrons (2 in each of the three orientations) and a 3s orbital can hold 2 electrons.
- **Energy**: The 3s orbital has more energy than the 2p orbital in most cases due to the Aufbau principle.

3p and 3d orbitals

- **Drawing**: A 3p orbital is similar in shape to a 2p orbital but larger, and a 3d orbital has a more complex shape with five different orientations.
- **Electron capacity**: A 3p orbital can hold 6 electrons and a 3d orbital can hold 10 electrons.
- **Energy**: The 3d orbital has more energy than the 3p orbital.

4d, 5p, and 6s orbitals

- **Drawing**: The 4d orbital has a complex shape with five orientations, the 5p orbital has a dumb - bell shape with three orientations, and the 6s orbital is spherical.
- **Electron capacity**: 4d can hold 10 electrons, 5p can hold 6 electrons, and 6s can hold 2 electrons.
- **Energy**: In general, the order of energy is $6s<4d<5p$.

Highest - energy orbital

- For any element, the highest - energy orbital is the valence orbital. This information is important because it determines the chemical reactivity of the element. The periodic table is structured based on the filling of orbitals. The rows (periods) correspond to the principal quantum number ($n$) of the outermost occupied orbital, and the columns (groups) are related to the number of valence electrons.

Answer:

Please refer to the above - step - by - step explanations for answers to each part of the question.