Which Brick Bond is right for your masonry project? Brick bonding is an industry term for the uniform pattern in which brickwork is laid and maximises the strength of the structure. Whilst its primary purpose is structural, the brick bond can also strongly influence the appearance of the façade and provide aesthetic character to many properties.

It’s important to consider these factors when initially deciding on your brickwork, as they can have an impact on the overall appearance of the build.We offer expert advice on the right brick bond for your project—simply and we’ll do the rest. Below you can see the most common variations of brick bond used in masonry : Stretcher Bond

Stretcher bond is the most typical laid bond in the UK. The pattern is laid with the stretcher course sitting halfway over the joints of the courses in the row below. While not particularly strong, it is a time and cost-effective way of laying brickwork. First used in 1631, it became popular in the late 18th century. Header Bond Header bond is similar to stretcher bond, however it features courses of headers. In header bonds, all bricks in each course are placed as headers on the faces of the walls. English Bond English bond is one of the oldest forms of brick bonding. It became common in the 1450s and was the standard type of brickwork for British houses until the late 17th century. English bond brickwork combines alternate courses of stretchers and headers. Flemish Bond Flemish bond is another traditional pattern where stretchers and headers are laid alternately in a single course. Flemish bond is attractive aesthetically, but is weaker than English bond for load bearing wall construction. It is often used for walls that are two bricks thick. Stack Bond In Stack bond pattern, the bricks are laid directly on top of one another with all joints aligned. The bricks are stacked vertically down the wall which results in minimal bonding, therefore this brickwork pattern has less structural integrity than others. This pattern is often used for decorative purposes. English Garden Wall Bond English Garden Wall bond constitutes three rows of stretchers to one row of headers. It is very rarely found on buildings outside the north of the UK, where it is abundant and particularly prevalent on the east coast. It was used from the late 18th century onwards, and was also used occasionally for garden walls. It uses fewer facing bricks than English bond. Flemish Garden Wall Bond Flemish Garden Wall bond, also known as Sussex bond, includes three stretchers to one header in each row. Ironically, this bond was in fact rarely used on garden walls historically. It is most common in West Sussex and Hampshire where it may be found on up to 10% of historic buildings.

Which bond is stronger English or Flemish?

Which of the following is a type of bond which consists of a Free 10 Questions 10 Marks 7 Mins Explanation: Different type of bonding in Brick masonry:

English bond Flemish bond Stretcher bond Header bond

English Bond:

It is the arrangement of bonding that consists of alternate courses of stretcher and header placed one over other, In order to break the alignment of vertical joints to be in the same straight line queen closer is placed next to the quoin header in each alternate course. Header courses must not start from queen closer as it is liable to get displace off. A lap of one-fourth brick is available for each stretcher over the header in the course below it. For the wall having the thickness in the odd multiples of half brick thick, each course shows a stretcher on one face and a header on the other face.

Flemish Bond:

It is the arrangement of bonding that consists of an alternate header and stretcher in each course, The header in each alternate course is centered over the stretcher in the course below it. In order to break the alignment of the vertical joint to be in the same straight line queen closer is placed next to the quoin header. For walls having a thickness greater than 1.5 brick thick, an English bond is found to be stronger than a Flemish bond, however, a Flemish bond renders a higher aesthetic appearance than an English bond, Flemish bond is more economical than the English bond.

Stretcher bond:

It is the arrangement of bonding that consists of a stretcher in each course, In order to break the alignment of the vertical joint to be in the same straight line each alternate course started with the half-bat. A lap of half-brick is available for each stretcher in all the courses. This bond is provided when a half brick thick wall is required.

Header bond:

It is the arrangement of bonding that consists of a header in each course, In order to break the alignment of the vertical joint to be in the same straight line each alternate course started in the quarter bat. A lap of half-width is available for each header in all the courses. This bond is generally provided in foundation work, in order to uniformly distributed the transverse load.

India’s #1 Learning Platform Start Complete Exam Preparation Daily Live MasterClasses Practice Question Bank Mock Tests & Quizzes Trusted by 3.4 Crore+ Students : Which of the following is a type of bond which consists of a

Which bond is the strongest bond in construction?

English Bond – An English bond can be constructed for almost all wall thicknesses. This bond is the strongest among all other bonds. This bond consists of alternate courses of headers and stretchers as shown in figure-1. Fig.1. English Bond in Brick Masonry Also Read: Types of Bonds in Brick Masonry Construction As shown in the figure above, the vertical joints come over each other. This is also followed by the vertical joints of the stretcher course. The vertical joints are broken to avoid the joints to form inline, by using a queen closer. Fig.2. English Bond for One and One and a Half brick Wall Thickness Fig.3. English Bond for Two and Two and a Half brick Wall Thickness

What is the strongest weak bond?

Therefore, the order from strongest to weakest bond is Ionic bond > Covalent bond > Hydrogen bond > Vander Waals interaction.

Which bond is hardest to break?

Eilisha Joy Bryson August 16, 2007 MISEP Chem 512 – Jacobs Enduring Understanding Essay Enduring Understanding #4 – The bonding within a molecule determines its shape and polarity, and therefore its interactions and reactions with other molecules. Intermolecular interactions are central to the structure and function of the biochemical systems, and the extent and rate of biochemical reactions govern all cellular functions.

Both interactions and reactions can be understood by analyzing energetic stability of the molecules and bonds. Two types of bonds are pertinent to this Enduring Understanding. The first is due to intra molecular forces that make chemical covalent bonds, either polar or non-polar. Because of the octet rule only certain arrangements of bonds will make a stable molecule, consequently giving a molecule its geometric shape.

Using the type of covalent bond, the presence of lone pairs, and the symmetry of the shape of the molecule, you can determine if the entire molecule is polar or not (which is different than polar bonding). The polarity of the molecule determines the forces occurring between it and other molecules.

• These inter molecular forces are basically weak bonds, but are essential in holding molecules together.
• Non-polar molecules have the weakest attractions called London forces.
• Polar molecules have stronger inter molecular attractions, called dipole-dipole forces.
• The strongest inter molecular force is a special type of dipole-dipole interaction called a hydrogen bond, formed between a molecule that contains a hydrogen atom and a molecule that contains a nitrogen, oxygen, or fluorine atom, which are highly electronegative.

Intra molecular covalent bonds are the hardest to break and are very stable, being about 98% stronger than intermolecular bonds. The covalent and inter molecular bonds discussed above result in numerous structures and functions of biochemical systems.

1. This is described below using the multi-structures of proteins.
2. The primary structure of the protein is the long amino acid chain, and it is formed by intra molecular covalent bonds.
3. Enzymes fold the primary structure, creating regions of repeating patterns, a -helix and b -sheets being the most popular.

The folds are held together and maintain their shape due to the inter molecular force of hydrogen bonds. There can be several differently shaped regions making up the secondary structure. The secondary structure then folds onto itself creating a 3-dimensional shape called the tertiary structure.

• This is held together and maintains its shape due to all of the inter molecular forces: London, dipole-dipole and hydrogen bonds, as well as ionic and disulfide bonds which are intra molecular.
• The sequence of the amino acids determines the structures of the protein and the structures result in the proteins function.

Last summer in our Biology course, we learned about the mechanism of hormones. Dr. Waldrons notes read, It begins with the binding of a hormone molecule to a specific hormone receptor, which is a protein with a binding site which specifically matches the shape and electrical charge distribution of the particular hormone molecule.

Focusing on the hormone receptor protein, you can see here how shape relates to function. An excellent example that we looked at during this class was with a protein whose job was to destroy blood cells. The proteins shape, which consisted of polar and non-polar regions, allowed it to take advantage of both the lipid and water-based properties of the cell.

While researching such proteins on the internet an article described a prion protein that was responsible for destroying brain cells. The protein Prp takes on an unexpected amyloid fold that consists of tight b -sheets that are difficult to penetrate, changing it into PrPsc.

• These incorrect folds cause the protein to turn brain cells into sponge-like holes.
• Prion is found in patients cells who had various diseases, such as Alzheimer’s and Down’s syndrome.
• Simply changing the shape of a region of the protein results in a new and dangerous function.
• Reactions change the covalent bonds within a molecule, breaking old bonds and making new ones.

If there is more energy released when the bonds form between the products compared to the amount of energy absorbed to break the bonds between reactants, then the reaction is termed exothermic, and heat is given off, and the products are more stable than the reactants. References : http://people.sps.lane.edu/jtyser/chem/Quiz/Unit12Test.html (endothermic potential energy diagram) http://www.simsoup.info/SimSoup/Potential_Energy_Profile.png (exothermic potential energy diagram) Cocchetto, A. (2004). Amyloids: A Basic Primer.

What is the strongest bond strength?

Covalent Bonds – Another type of strong chemical bond between two or more atoms is a covalent bond, These bonds form when an electron is shared between two elements. Covalent bonds are the strongest (*see note below) and most common form of chemical bond in living organisms.

The hydrogen and oxygen atoms that combine to form water molecules are bound together by strong covalent bonds. The electron from the hydrogen atom shares its time between the hydrogen atom and the oxygen atom. In order for the oxygen atom to be stable, two electrons from two hydrogen atoms are needed, hence the subscript “2” in H 2 O.

H 2 O means that there are 2 hydrogen atoms bonded to 1 oxygen atom (the 1 is implied below the O in the chemical formula). This sharing makes both the hydrogen and oxygen atoms more chemically stable. There are two types of covalent bonds: polar and nonpolar (Figure 3).

1. Nonpolar covalent bonds form between two atoms that share the electrons equally so there is no overall charge on the molecule.
2. For example, an oxygen atom can bond with another oxygen atom.
3. This association is nonpolar because the electrons will be equally shared between each oxygen atom.
4. Another example of a nonpolar covalent bond is found in the methane (CH 4 ) molecule.

The carbon atom shares electrons with four hydrogen atoms. The carbon and hydrogen atoms all share the electrons equally, creating four nonpolar covalent bonds (Figure 3). In a polar covalent bond, the electrons shared by the atoms spend more time closer to one atom than to the other.

Because of the unequal distribution of electrons between the atoms, a slightly positive (δ+) or slightly negative (δ–) charge develops. The covalent bonds between hydrogen and oxygen atoms in water are polar covalent bonds. The shared electrons spend more time near the oxygen than they spend near the hydrogen.

This means that the oxygen has a small negative charge while the hydrogens have a small positive charge. Figure 3 The water molecule (left) depicts a polar bond with a slightly positive charge on the hydrogen atoms and a slightly negative charge on the oxygen. Examples of nonpolar bonds include methane (middle) and oxygen (right).

Which single bond is strongest?

Sigma bonds are strong bonds compared to pi bonds where participating orbitals undergo direct overlapping.

Why is English bond strongest?

English Bond – This is another common type of bond that you see used on a lot of British buildings and is easy to spot since it’s such a distinctive pattern. The English brick bond alternates rows of headers with rows of stretchers. This type of wall-building uses more bricks than a stretcher bond, so is rarely used for largescale residential developments, but it is often considered one of the best and strongest brick bond designs around.

What are the two strongest types of bonds?

Covalent and ionic bonds are both typically considered strong bonds. However, other kinds of more temporary bonds can also form between atoms or molecules. Two types of weak bonds often seen in biology are hydrogen bonds and London dispersion forces.

What makes a brick wall strong?

Today’s Wonder of the Day was inspired by Ella. Ella Wonders, ” What are bricks made of? ” Thanks for WONDERing with us, Ella! We were walking leisurely through the fields of the Wonderopolis farm the other day when we came upon the barn and caught a snippet of three little pigs having the following conversation : Little Pig #1: Hey! I was thinking about building a house.

• Any ideas of what I should use? Little Pig #2: Well, you could use straw,
• Hee hee Little Pig #3: Yeah! Yeah! Or sticks.
• Yeah, use sticks! Ha ha ha! Little Pig #1: What’s so funny? Am I missing something here? Little Pig #2: Are you serious? Little Pig #3: Yeah, please tell us you’re joking! Little Pig #1: I don’t get it.

Would someone please tell me what’s so funny? Little Pig #2: Umdoesn’t this conversation remind you of a familiar story? Little Pig #3: Yeah, you know, with three little pigs and a Big Bad Wolf ? Little Pig #1: You mean that story’s true? Yikes! I guess I should use bricks then.

Little Pig #2: Of course, it’s true. And, yes, you should definitely use bricks. Little Pig #3: The hardware store over on Route 7 has them on sale this week Little Pig #1: Thanks for the advice ! (wanders off) Little Pig #2: You’re welcome. (shakes head) Little Pig #3: That dude is totally going to be bacon by the end of the week! We don’t know about you, but we hope that Little Pig #1 heeds the advice of the other two little pigs.

Building a house of straw or sticks just isn’t the smart thing to do when bricks are available! The first human beings probably used wood and stone to build the first structures. However, using bricks probably wasn’t far behind. Scientists know that bricks were made long before written history.

1. And they’re still very popular today, thousands upon thousands of years later.
2. The main ingredient in bricks is clay, which comes from the ground.
3. Clay results from the break-up of rock over time.
4. Weather, chemical reactions, volcanoes, and even glaciers can grind rock into a fine powdery earth called clay over long periods of time.

When it is wet, clay can be shaped easily by hand. Early clay bricks were probably made by shaping the clay into a suitable shape for a building block and then allowing it to dry in the sun. Today, bricks are mainly made by machines. Clay is pressed into a mold and then baked at over 1,000 degrees Fahrenheit until the brick is very hard.

Bricks are often made by creating large columns that are subsequently cut into smaller individual bricks. A large brick factory in England can produce as many as 16 million bricks in a single week! Many bricks are naturally red in color because of the presence of iron in the clay used to make them. Bricks of different colors can be made by adding other substances to the clay before baking them.

So why is brick such a great building material? Not only can it withstand the huffs and puffs of the Big Bad Wolf, but it’s also basically maintenance free. Over long periods of time, it doesn’t break, rot, or need to be painted. Bricks also will not be eaten by termites or other insects that might otherwise feast on a house made of straw or sticks.

Why is brick so strong? When fired at extremely high temperatures, the clay particles fuse together to form a super-strong bond that makes clay bricks into metamorphic rocks. Clay bricks are stronger than concrete and many other building materials. When combined in an interlocking pattern with other bricks and held together by a cement called mortar, bricks make sturdy structures that can survive for hundreds, if not thousands, of years with very little maintenance,

For example, the Great Wall of China was built over two thousand years ago with nearly 4 billion bricks!

What is the strongest and shortest bond?

Applying the above points, we get to know that the triple bonds are strongest and thus the shortest among single, double and triple bonds.

What is the second strongest bond?

Therefore, the order of strength of bonds from the strongest to weakest is; Ionic bond > Covalent bond > Hydrogen bond > Van der Waals interaction.

What are the 4 types of bonds?

crystal – Types of bonds The properties of a can usually be predicted from the valence and bonding preferences of its atoms. Four main bonding types are discussed here: ionic, covalent, metallic, and molecular. Hydrogen-bonded solids, such as, make up another category that is important in a few crystals.

There are many examples of solids that have a single bonding type, while other solids have a mixture of types, such as covalent and metallic or covalent and ionic. exhibits ionic bonding. The has a single in its outermost shell, while needs one electron to fill its outer shell. donates one to chlorine, forming a sodium (Na + ) and a chlorine (Cl − ).

Each ion thus attains a closed outer shell of electrons and takes on a spherical shape. In addition to having filled shells and a spherical shape, the ions of an ionic solid have integer valence. An ion with positive valence is called a, In an ionic solid the cations are surrounded by ions with negative valence, called,

Similarly, each anion is surrounded by cations. Since opposite charges attract, the preferred bonding occurs when each ion has as many neighbours as possible, consistent with the ion radii. Six or eight nearest neighbours are typical; the number depends on the size of the and not on the bond angles. The alkali halide crystals are binaries of the AH type, where A is an alkali ion (lithium, sodium, potassium, rubidium, or cesium) and H is a halide ion (fluorine, chlorine, bromine, or iodine).

The crystals have bonding, and each ion has six or eight neighbours. Metal ions in the (magnesium, calcium, barium, and strontium ) have two electrons in their outer shells and form divalent cations in ionic crystals. The (oxygen, sulfur, selenium, and tellurium) need two electrons to fill their outer p -shell.

1. Electron shells are divided into subshells, designated as s, p, d, f, g, and so forth.
2. Each subshell is divided further into orbitals.) Two electrons are transferred from the cations to the anions, leaving each with a closed shell.
3. The earth chalcogenides form crystals such as (BaO), (CaS), barium selenide (BaSe), or strontium oxide (SrO).

They have the same structure as sodium chloride, with each atom having six neighbours. can be combined with various cations to form a large number of ionically bonded solids.,,, and a few other elements form covalently bonded solids. In these elements there are four electrons in the outer -shell, which is half filled.

1. The s p -shell is a hybrid formed from one s and one p subshell.) In the an atom shares one (outer-shell) electron with each of its four nearest neighbour atoms.
2. The bonds are highly directional and prefer a tetrahedral arrangement.
3. A covalent bond is formed by two —one from each atom—located in orbitals between the ions.

Insulators, in contrast, have all their electrons within shells inside the atoms. The perpetual spin of an electron is an important aspect of the covalent bond. From a vantage point above the spinning particle, counterclockwise rotation is designated spin-up, while clockwise rotation is spin-down.

A fundamental law of is the, which states that no two electrons can occupy the same point in space at the same time with the same direction of spin. In a covalent bond two electrons occupy the same small volume of space ( i.e., the same orbital) at all times, so they must have opposite spin: one up and one down.

The exclusion principle is then satisfied, and the resulting bond is strong. In the carbon atoms are arranged in parallel sheets, and each atom has only three near neighbours. The covalent bonds between carbons within each layer are quite strong and are called bonds.

The fourth in carbon has its orbital perpendicular to the plane. This orbital bonds weakly with the similar orbitals on all three neighbours, forming bonds. The four bonds for each carbon atom in the graphite structure are not arranged in a tetrahedron; three are in a plane. The planar arrangement results in strong bonding, although not as strong as the bonding in the configuration.

The bonding between layers is quite weak and arises from the ; there is much slippage parallel to the layers. Diamond and graphite form an interesting contrast: diamond is the hardest material in nature and is used as an, while graphite is used as a lubricant.

Besides the elemental semiconductors, such as silicon and germanium, some binary crystals are covalently bonded. has three electrons in the outer shell, while lacks three. (GaAs) could be formed as an insulator by transferring three electrons from gallium to arsenic; however, this does not occur. Instead, the bonding is more covalent, and gallium arsenide is a covalent,

The outer shells of the gallium atoms contribute three electrons, and those of the arsenic atoms contribute five, providing the eight electrons needed for four covalent bonds. The centres of the bonds are not at the midpoint between the ions but are shifted slightly toward the arsenic.

Such bonding is typical of the — i.e., those consisting of one element from the third column of the and one from the, Elements from the third column (boron, aluminum, gallium, and indium) contribute three electrons, while the fifth-column elements (nitrogen, phosphorus, arsenic, and antimony) contribute five electrons.

All III–V semiconductors are covalently bonded and typically have the structure with four neighbours per atom. Most common favour this arrangement. The factor that determines whether a binary crystal will act as an or a semiconductor is the valence of its constituent atoms.

That donate or accept one or two valence electrons form insulators. Those that have three to five valence electrons tend to have covalent bonds and form semiconductors. There are exceptions to these rules, however, as is the case with the IV–VI semiconductors such as lead sulfide. Heavier elements from the fourth column of the periodic table (germanium, tin, and lead) with the chalcogenides from the sixth row to form good binary semiconductors such as germanium telluride (GeTe) or tin sulfide (SnS).

They have the sodium chloride structure, where each atom has six neighbours. Although not tetrahedrally bonded, they are good semiconductors. Filled atomic shells with -orbitals have an important role in covalent bonding. Electrons in atomic orbits have ( L ), which is quantized in integer ( n ) multiples of h : L = n h,

Electron orbitals with n = 0 are called -states, with n = 1 are -states, and with n = 2 are d -states. and ions have one valence electron outside their closed shells. The outermost filled shell is a d -state and affects the bonding. Eight crystals are formed from the copper and, Three (AgF, AgCl, AgBr) have the sodium chloride structure with six neighbours.

The other five (AgI, CuF, CuCl, CuBr, CuI) have the zinc blende structure with four neighbours. The bonding in this group of solids is on the borderline between covalent and ionic, since the crystals prefer both types of bonds. The halides exhibit somewhat different behaviour.

1. The alkali metals are also monovalent cations, but their halides are strictly ionic.
2. The difference in bonding between the alkali metals on the one hand and silver and copper on the other hand is that silver and copper have filled d -shells while the alkalis have filled p -shells.
3. Since the d -shells are filled, they do not covalently bond.

This group of electrons is, however, highly polarizable, which influences the bonding of the valence electrons. Similar behaviour is found for and, which have two valence electrons outside a filled d -shell. They form binary crystals with the chalcogenides, which have tetrahedral bonding.

In this case the covalent bonding seems to be preferred over the, In contrast, the alkaline earth chalcogenides, which are also divalent, have outer p -shells and are ionic. The zinc and cadmium chalcogenides are covalent, as the outer d -shell electrons of the two cations favour covalent bonding. Metallic bonds fall into two categories.

The first is the case in which the are from the -shells of the metal ions; this bonding is quite weak. In the second category the valence electrons are from partially filled d -shells, and this bonding is quite strong. The d -bonds dominate when both types of bonding are present.

1. The are bonded with s p -electrons.
2. The electrons of these metal atoms are in filled atomic shells except for a few electrons that are in unfilled s p -shells.
3. The electrons from the unfilled shells are detached from the metal ion and are free to wander throughout the crystal.
4. They are called, since they are responsible for the electrical conductivity of metals.

Although the conduction electrons may roam anywhere in the crystal, they are distributed uniformly throughout the entire solid. Any large imbalance of charge is prevented by the strong electrical attraction between the negative electrons and the positive ions, plus the strong repulsion between electrons.

• The phrase electron correlation describes the correlated movements of the electrons; the motion of each electron depends on the positions of neighbouring electrons.
• Electrons have strong short-range order with one another.
• Correlation ensures that each unit cell in the crystal has, on the average, the number of electrons needed to cancel the positive charge of the cation so that the unit cell is electrically neutral.

is the energy gained by arranging the atoms in a crystalline state, as compared with the state. Insulators and semiconductors have large energies; these solids are bound together strongly and have good mechanical strength. Metals with electrons in s p -bonds have very small cohesive energies.

• This type of is weak; the crystals are barely held together.
• Single crystals of simple metals such as are mechanically weak.
• At room the crystals have the mechanical consistency of warm butter.
• Special care must be used in handling these crystals, because they are easily distorted.
• Metals such as magnesium or aluminum must be alloyed or polycrystalline to have any mechanical strength.

Although the simple metals are found in a variety of structures, most are in one of the three closest-packed structures: fcc, bcc, and hcp. calculations show that the cohesive energy of a given metal is almost the same in each of the different crystal arrangements; therefore, crystal arrangements are unimportant in metals bound with electrons from s p -shells.

1. A different type of metallic bonding is found in, which are metals whose atoms are characterized by unfilled d -shells.
2. The d -orbitals are more tightly bound to an ion than the s p -orbitals.
3. Electrons in d -shells do not wander away from the ion.
4. The d -orbitals form a covalent bond with the d -orbitals on the neighbouring atoms.

The bonding of d -orbitals does not occur in a tetrahedral arrangement but has a different directional preference. In metals the bonds from d -orbitals are not completely filled with electrons. This situation is different from the tetrahedral bonds in semiconductors, which are filled with eight electrons.

In metals the covalent bonds formed with the d -electrons are much stronger than the weak bonds made with the s p -electrons of simple metals. The cohesive energy is much larger in transition metals. Titanium, iron, and tungsten, for example, have exceptional mechanical strength. Crystal arrangements are important in the behaviour of the transition metals and occur in the close-packed fcc, bcc, or hcp arrangements.

: crystal – Types of bonds

Which bond is easiest to break?

The hydrogen bond is the weakest bond among the covalent, ionic, and metallic bonds. A hydrogen bond occurs as a weak attraction between the molecules because it depends on a temporary imbalance in electron distribution.

Which of the following is the weakest bond?

Ionic bonds and covalent bonds are strong while hydrogen bonds and London forces are weak. So, the weakest force is London force.

What is the greatest weakness of a brick structure?

2. Lack of Adaptability to Climate Changes – Brick is a very rigid material and therefore doesn’t have very much flex or give to it. All climates experience changes in temperature, but some regions have much more intense swings in temperatures or seasonal changes. Brick and mortar simply can’t expand and contract when this occurs repeatedly.

Eventually the brick and mortar will wear down, crack, or otherwise gradually fail. Additionally, home in regions where earthquakes and shifting are common will find out sooner or later that brick simply won’t shift with the home’s foundation. Fiber cement is capable of expansion and contraction during significant temperature swings, allowing it to bend with the home rather than crack against the pressure.

It’s slight flexibility also helps when the earth and thus the home’s foundation shifts naturally. While any significant weather catastrophes or earthquakes certainly can wreak havoc on even the most durable siding material, fiber cement is still going to outlast brick.

Which compound has the weakest bond?

The bond in lithium molecule is weakest.