How Do Atoms Bond | Properties of Matter | Chemistry | FuseSchool
Summary
TLDRThis 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
🔬 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.
Mindmap
Keywords
💡Structure and Bonding
💡Molecular Covalent Bonding
💡Giant Covalent
💡Metallic Bonding
💡Ionic Bonding
💡Effective Nuclear Charge
💡Noble Gases
💡Periodic Table
💡Reactive Metals
💡Reactive Non-metals
💡Shielding Effect
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
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