Question

What is the expected ground-state electron configuration for the element with one unpaired \(5 p\) electron that forms a covalent compound with fluorine?

Short answer

The ground-state electron configuration for the element with one unpaired 5p electron that forms a covalent compound with fluorine is antimony (Sb) and its electron configuration is: \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{3}\] Antimony forms the covalent compound SbF3 with fluorine by sharing electrons.

Step-by-step solution

Identifying the element with an unpaired 5p electron

To identify the element, we need to find the one with an unpaired 5p electron. In the periodic table, the elements in the p-block have p-electrons. The 5p orbital can hold up to 6 electrons. The element with only one unpaired electron in the 5p orbital must have 5 electrons in total: 2 in 5s and 3 in 5p orbitals. This element is antimony (Sb) with atomic number 51.

Determining the electron configuration of antimony

Now that we've identified the element as antimony (Sb), we can write its electron configuration. The electron configuration of an element tells us how the electrons are distributed among various atomic orbitals. The electron configuration of antimony with an atomic number of 51 is: \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{3}\] This configuration represents the ground-state electron distribution for Sb.

Understanding how antimony forms a covalent bond with fluorine

Antimony (Sb) forms a covalent compound with fluorine (F). In a covalent bond, the elements share electrons to complete their respective octets. Fluorine, with an electron configuration of \(1s^{2}2s^{2}2p^{5}\), has seven valence electrons and needs one more to complete its octet. Antimony, with its electron configuration ending in 5p^3, has three valence electrons. By sharing one valence electron with fluorine (which needs one electron to complete its octet), antimony will still have two unpaired electrons. In order to complete its octet, antimony can share these two unpaired electrons with two more fluorine atoms. Thus, they form the covalent compound SbF3. So, the expected ground-state electron configuration for the element with one unpaired 5p electron that forms a covalent compound with fluorine is: \[1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{3}\]

Key concepts

Ground-state Electron Distribution

To get a handle on the concept of ground-state electron distribution, let's think of it as a roadmap that shows us where the electrons are living in an atom when it's not excited. Just like you might head home after a long day, electrons have their own 'homes' in an atom that are called orbitals.

When we talk about ground state, we're picturing the electrons in their most relaxed state, with no extra energy pumping them up to higher energy levels. They fill up their orbitals in a really specific order, kind of like how you fill up a cup of water from the bottom to the top, not the middle out. This order helps us predict a lot about an element's chemical behavior, like how it might bond with other elements.

P-block Elements

Meet the Neighborhood

Imagine walking into a neighborhood where all the houses have a similar style. That's kind of like stumbling into the p-block section of the periodic table. These elements have their valence electrons hanging out in p-orbitals, which are kind of like three-dimensional dumbbell-shaped zones.

These p-block residents include a diverse bunch. Some are metals, some nonmetals, and others are metalloids, which are elements that can't decide if they're tough like metals or more nonmetallic in nature. But what they all have in common is that their chemistry is heavily influenced by those p-orbital electrons that can participate in bonding, and they play a big role in the materials and technologies we use every day.

Covalent Bonding

Now let’s dive into the realm of sharing, which is what covalent bonding is all about. It’s like two friends sharing fries; each atom shares its electrons with another to fill up their respective electron dance cards or, more scientifically, their outer shells.

When atoms come together in a covalent bond, they're searching for stability, and they find it through this sharing. It's a pretty democratic process because the electrons are shared equally or unequally based on the atom's electronegativity. This sharing creates a powerful connection that's tough to break, and it's the reason why substances like water and the air we breathe exist.

Octet Rule

The Ultimate Goal

The octet rule is like the ultimate success rule for atoms in the game of chemistry. Atoms aim to have eight electrons in their outermost shell because this full house brings them bliss and stability.

Think of it like a party where everyone wants to have eight people in their group for the perfect balance of fun. Most atoms will do whatever they can—sharing, giving, or taking electrons—to reach that magic number, just like the element antimony does when it forms bonds with fluorine atoms to become a well-rounded and stable SbF3 molecule.