How Do Atoms Bond | Properties of Matter | Chemistry | FuseSchool

Summary

This two-part video delves into the four fundamental types of chemical bonding: molecular, covalent, giant covalent, and ionic. It explains that atoms bond to fill their outer electron shells, with non-metals holding onto electrons more tightly than metals. The video uses the periodic table to illustrate the transition from metallic to non-metallic elements and how this influences bonding. It sets the stage for part two, where it will detail the specific bonding types formed between elements, exemplified by the reaction between cesium and fluorine to form cesium fluoride.

Takeaways

• 🔬 There are only four possible structures that form when elements bond: molecular, covalent, giant covalent, metallic, and ionic bonding.
• ⚛️ Noble gases do not easily form bonds due to their full outer electron shells.
• 💡 Electrons in the inner shells shield the outer electrons from the full nuclear charge, creating an effective nuclear charge that influences bonding.
• 🌟 Non-metals with nearly full outer shells hold onto their electrons more strongly than metals with nearly empty shells.
• 🔁 Atoms bond if there is space in their outer shells for additional electrons from other atoms.
• 📊 The periodic table can be visualized as a transition from metallic to non-metallic elements, with reactive metals on one end and non-metals on the other.
• 🔄 Elements at the extremes of the metallic and non-metallic spectrum, like cesium and fluorine, tend to form ionic bonds, resulting in stable compounds like caesium fluoride.
• 🔗 The periodic table can be rearranged to show a gradient from the most metallic to the most non-metallic elements, helping to predict bonding types.
• 🧬 In part two of the video, it will be shown that the combination of elements can lead to only four types of bonding, which will be further explained.
• 🔬 The structure of elements and their bonding properties are closely related to their position and properties on the periodic table.

Q & A

Why do noble gases not easily form bonds?

Noble gases do not easily form bonds because they have full outer electron shells, which makes them stable and less likely to engage in bonding.

What is the role of inner electron shells in bonding?

Inner electron shells shield some of the nuclear charge from the outer shell electrons, which affects how strongly the outer electrons are held by the nucleus and their tendency to bond.

Why do non-metals hold onto their electrons more strongly than metals?

Non-metals hold onto their electrons more strongly because they have nearly full outer electron shells, whereas metals have nearly empty outer shells and are more willing to lose or share electrons.

How does the effective nuclear charge influence bonding?

The effective nuclear charge, which is the net positive charge felt by the outer electrons, influences bonding by determining how strongly atoms attract electrons from other atoms.

What is the significance of hydrogen's position in the periodic table?

Hydrogen is unique in the periodic table as it has a half-filled shell of electrons and is placed in group 1, 4, and 7, reflecting its dual nature in bonding.

How does the periodic table arrangement relate to the metallic and non-metallic properties of elements?

The periodic table arranges elements from the most metallic, like cesium, to the most non-metallic, like fluorine, with elements in between showing a gradual change in their metallic to non-metallic properties.

What is the result of the reaction between cesium and fluorine?

The reaction between cesium, a highly metallic element, and fluorine, a highly non-metallic element, results in the formation of the stable white salt cesium fluoride.

What are the four possible types of bonding mentioned in the script?

The script alludes to four types of bonding: molecular, covalent, giant covalent, and ionic bonding, which will be explained in more detail in part two of the video.

Why do atoms bond with other atoms?

Atoms bond with other atoms to fill their outer electron shells, achieving a stable electron configuration similar to that of noble gases.

How does the arrangement of elements in the periodic table influence the types of compounds formed?

The arrangement of elements in the periodic table, from metallic to non-metallic, influences the types of compounds formed, as elements tend to bond with others that can help them achieve a stable electron configuration.

What can be inferred about the bonding behavior of elements in the middle of the periodic table?

Elements in the middle of the periodic table, like silicon and germanium, exhibit properties of both metals and non-metals, and their bonding behavior is not as straightforward as the elements at the extremes.

Outlines

00:00

🔬 Structure and Bonding Overview

This segment introduces the concept of bonding in elements and compounds, explaining that there are only four possible structures formed when elements bond: molecular, covalent, giant covalent, metallic, and ionic. It emphasizes that atoms bond when there is space in their outer electron shells for more electrons, which is not the case for noble gases with full outer shells. The explanation includes the role of effective nuclear charge, which influences how strongly atoms hold onto their electrons, with non-metals holding onto their electrons more tightly than metals. The video also touches on the periodic table, highlighting the positions of reactive metals and non-metals, and how elements transition from metallic to non-metallic properties. The discussion sets the stage for part two, which will delve into the four types of bonding.

Keywords

💡Structure and Bonding

Structure and bonding refer to the arrangement of atoms and the forces that hold them together in molecules and compounds. In the context of the video, these concepts are central to understanding why only four types of bonding are possible. The video script discusses how atoms with different electron configurations can bond in different ways, leading to the formation of various structures.

💡Molecular Covalent Bonding

Molecular covalent bonding is a type of chemical bond where atoms share electrons to achieve a stable electron configuration. The video script explains that when elements bond, they form structures based on their electron needs, and molecular covalent bonding is one such structure that forms when electrons are shared between atoms.

💡Giant Covalent

Giant covalent structures are formed when a large number of atoms are bonded together in a network by covalent bonds. This type of structure is seen in materials like diamond, where each carbon atom is covalently bonded to four other carbon atoms, creating a rigid and strong lattice. The video script mentions this as one of the possible structures that can form when elements bond.

💡Metallic Bonding

Metallic bonding is a type of chemical bond that holds atoms together in a metal. It involves a 'sea' of delocalized electrons that are shared among a lattice of positively charged metal ions. The video script points out that metallic elements, which have nearly empty outer shells, are prone to form metallic bonds, as seen in elements like sodium.

💡Ionic Bonding

Ionic bonding occurs when electrons are transferred from one atom to another, resulting in the formation of oppositely charged ions that are attracted to each other. The video script uses the example of cesium fluoride, where the reactive metal cesium donates an electron to the reactive non-metal fluorine, forming a stable ionic compound.

💡Effective Nuclear Charge

Effective nuclear charge is the net positive charge experienced by the valence electrons of an atom, taking into account the shielding effect of inner electrons. The video script explains that non-metals, like chlorine, with nearly full outer shells experience a higher effective nuclear charge, making them hold onto their electrons more tightly and less likely to form bonds.

💡Noble Gases

Noble gases are a group of chemical elements with full valence electron shells, making them chemically stable and unreactive. The video script notes that noble gases do not easily form bonds because their outer electron shells are complete, and they are not inclined to gain or lose electrons.

💡Periodic Table

The periodic table is a tabular arrangement of chemical elements by their atomic number, electron configuration, and recurring chemical properties. The video script uses the periodic table to illustrate the transition from metallic to non-metallic elements and how this influences the types of bonding that elements can form.

💡Reactive Metals

Reactive metals are elements that readily lose electrons to form positive ions. The video script identifies a section of the periodic table where very reactive metals like potassium are located, indicating that these elements are likely to form ionic bonds with non-metals.

💡Reactive Non-metals

Reactive non-metals are elements that tend to gain electrons to achieve a full valence shell. The video script points out that elements like oxygen and chlorine are very reactive non-metals, which are more likely to form covalent bonds or accept electrons to form anions.

💡Shielding Effect

The shielding effect is the reduction in the attractive force exerted by the nucleus on an electron due to the presence of other electrons between the nucleus and the electron in question. The video script explains that this effect is crucial in determining the effective nuclear charge felt by the outer electrons, which in turn influences the bonding behavior of elements.

Highlights

There are only four possible structures that form when elements bond: molecular, covalent, giant covalent, metallic, and ionic bonding.

Noble gases with full outer electron shells do not easily form bonds.

Inner electrons shield some of the nuclear charge from the outer shell electrons.

In chlorine, the inner 10 electrons neutralize the effect of 10 protons, leaving the outer 7 electrons feeling an effective charge of 7+.

Sodium's outer electron feels an effective charge of only +1 due to the shielding effect of the inner electrons.

Non-metals with nearly full shells hold onto their electrons more strongly than metals with nearly empty shells.

Atoms bond if there is space in their outer shells for more electrons.

The periodic table can be arranged from the most metallic to the most non-metallic elements.

Hydrogen is unique, being in group 1, 4, and 7 of the periodic table.

Very reactive metals like potassium are found on one side of the periodic table.

Very reactive non-metals like oxygen and chlorine are found on the opposite side of the periodic table.

Elements in between the metals and non-metals on the periodic table have intermediate properties.

The reaction between cesium and fluorine, two extreme elements, forms the stable white salt caesium fluoride.

Compounds like brass, sulfur dioxide, sand, and salt fill the space between elements in the periodic table.

By considering reactions between pairs of elements, only four types of bonding are possible.

The video series will explain the bonding types in part two.

Transcripts

structure and bonding of elements and

compounds part one

this two-part video explains why there

are only four possible structures that

form when elements bond molecular

covalent giant covalent metallic and

ionic bonding

if you want to know more about each

individual bond you can click on these

videos

atoms bond if there is space in the

outer electron shells for more electrons

thus the noble gases with their full

outer shells don't easily form bonds

in an atom the inner complete shells of

negatively charged electrons are held

tightly by the positively charged

protons in the nucleus

however these inner electrons will

shield some of this nuclear charge from

the electrons in the outer shell which

will only feel this excess charge

thus in chlorine the inner 10 electrons

will cancel out or neutralize the effect

of 10 of the protons

so the outer 7 electrons feel an

effective charge of just 7 plus holding

them in their outer shell

sodium with 11 protons and 11 electrons

has also 10 in electrons leaving an

effective charge of only plus one to

hold its single outer electron thus we

see why non-metals with nearly full

shells hold on to their electrons more

strongly than metallic elements with

nearly empty shells we also see why

atoms bond if there is a space in their

outer shells electrons from other atoms

can be attracted in by this effective

nuclear charge but only until the shell

is full

so let's start with the periodic table

of elements omitting the noble gases and

this last row of radioactive elements

from our periodic table

note that hydrogen with its half-filled

shell of electrons heads up group four

as well as being in group one with its

one outer electron and group seven with

one electron missing

here are all the very reactive metals

like potassium

here are all the very reactive

non-metals like oxygen and chlorine

in between the elements gradually change

from being metallic to non-metallic with

some like silicon and germanium neither

one nor the other

if we twist the periodic table clockwise

and then squash it flat we pretty much

have the elements arranged from the most

metallic cesium

to the most non-metallic fluorine

when these two extreme elements react

they form the stable white salt caesium

fluoride we now have a triangular space

where all other combinations of elements

can be situated elements are along the

top and the space will be filled with

compounds like brass

sulfur dioxide sand and salt

by considering the reaction between

pairs of elements like this we will show

in part two of this video that there are

only four types of bonding possible