Chapter 8 Flashcards

Question

Covalent Bonding: Definition

Answer 1

- Covalent bonding occurs between two nonmetals - A covalent bond involves the electrostatic attraction between nuclei of two atoms and the bonding electrons of their outer shells - No electrons are transferred but only shared in this type of bonding - Non-metals are able to share pairs of electrons to form different types of covalent bonds - Sharing electrons in the covalent bond allows each of the 2 atoms to achieve an electron configuration similar to a noble gas - -----This makes each atom more stable

Answer 2

- Dot and cross diagrams are used to represent covalent bonding - They show just the outer shell of the atoms involved - To differentiate between the two atoms involved, dots for electrons of one atom and crosses for electrons of the other atom are used - Electrons are shown in pairs on dot-and-cross diagrams

Answer 3

Being able to accommodate more than 8 electrons in the outer shell

Answer 4

Accommodating less than 8 electrons in the outer shell means than the central atom -Some examples of this occurring can be seen with Period 3 elements

Answer 5

- In simple covalent bonds the two atoms involved shares electrons - Some molecules have a lone pair of electrons that can be donated to form a bond with an electron-deficient atom - ---An electron-deficient atom is an atom that has an unfilled outer orbital - So both electrons are from the same atom - This type of bonding is called dative covalent bonding or coordinate bond - An example of a dative bond is in an ammonium ion - ---The hydrogen ion, H+ is electron-deficient and has space for two electrons in its shell - ---The nitrogen atom in ammonia has a lone pair of electrons which it can donate to the hydrogen ion to form a dative covalent bond

Answer 6

dative covalent bonding - At high temperatures aluminium chloride can exist as a monomer (AlCl3) - ---The molecule is electron-deficient and needs to electrons complete the aluminium atom’s outer shell - At lower temperatures the two molecules of AlCl3 join together to form a dimer (Al2Cl6) - ----The molecules combine because lone pairs of electrons on two of the chlorine atoms form two coordinate bonds with the aluminium atoms

Answer 7

-A single covalent bond is formed when two nonmetals combine -Each atom that combines has an atomic orbital containing a single unpaired electron -When a covalent bond is formed, the atomic orbitals overlap to form a combined orbital containing two electrons -----This new orbital is called the molecular orbital The greater the atomic orbital overlap, the stronger the bond - Sigma (σ) bonds are formed by direct overlap of orbitals between the bonding atoms - Pi (π) bonds are formed by the sideways overlap of adjacent above and below the σ bond

Answer 8

- Sigma (σ) bonds are formed from the end-on overlap of atomic orbitals - S orbitals overlap this way as well as p orbitals - The electron density in a σ bond is symmetrical about a line joining the nuclei of the atoms forming the bond - The pair of electrons is found between the nuclei of the two atoms - The electrostatic attraction between the electrons and nuclei bonds the atoms to each other - single bonds

Answer 9

- Pi (π) bonds are formed from the sideways overlap of adjacent p orbitals - The two lobes that make up the π bond lie above and below the plane of the σ bond - This maximises overlap of the p orbitals - A single π bond is drawn as two electron clouds one arising from each lobe of the p orbitals - The two clouds of electrons in a π bond represent one bond containing two electrons by Double bond between atoms

Answer 10

- The hydrogen atom has only one s orbital | - The s orbitals of the two hydrogen atoms will overlap to form a σ bond

Answer 11

- Each carbon atom uses three of its four electrons to form σ bonds - Two σ bonds are formed with the hydrogen atoms - One σ bond is formed with the other carbon atom - The fourth electron from each carbon atom occupies a p orbital which overlaps sideways with another p orbital on the other carbon atom to form a π bond - This means that the C-C is a double bond: one σ and one π bond

Answer 12

- This molecule contains a triple bond formed from two π bonds (at right angles to each other) and one σ bond - Each carbon atom uses two of its four electrons to form σ bonds - One σ bond is formed with the hydrogen atom - One σ bond is formed with the other carbon atom - Two electrons are used to form two π bonds with the other carbon atom

Answer 13

- Hydrogen cyanide contains a triple bond - One σ bond is formed between the H and C atom (overlap of an sp C hybridised orbital with the 1s H orbital) - A second σ bond is formed between the C and N atom (overlap of an sp C hybridised orbital with a p orbital of N) - The remaining two sets of p orbitals of nitrogen and carbon will overlap to form two π bonds at right angles to each other

Answer 14

- Nitrogen too contains a triple bond - The triple bond is formed from the overlap of the s orbitals on each N to form a σ bond and the overlap of two sets of p orbitals on the nitrogen atoms to form two π bonds - These π bonds are at right angles to each other

Answer 15

- The p atomic orbitals can also overlap end-on to form σ bonds - In order for them to do this, they first need to become modified in order to gain s orbital character - The orbitals are therefore slightly changed in shape to make one of the p orbital lobe bigger - This mixing of atomic orbitals to form covalent bonds is called hybridisation - ---Mixing an s with three p orbitals is called sp3 hybridisation (each orbital has ¼ s character and ¾ p character) - ---Mixing an s with tw p orbital is called sp2 hybridisation - ---And mixing an s with one p-type orbitals formssp hybridised orbitals

Answer 16

- The bond energy is the energy required to break one mole of a particular covalent bond in the gaseous states - ---Bond energy has units of kJ mol-1 - The larger the bond energy, the stronger the covalent bond is

Answer 17

- The reactivity of a covalent bond is greatly influenced by: - ----The bond polarity - ----The bond strength - ----The bond type (σ/π)

Answer 18

- The bond length is internuclear distance of two covalently bonded atoms - It is the distance from the nucleus of one atom to another atom which forms the covalent bond - The greater the forces of attraction between electrons and nuclei, the more the atoms are pulled closer to each other - This decreases the bond length of a molecule and increases the strength of the covalent bond - Triple bonds are the shortest and strongest covalent bonds due to the large electron density between the nuclei of the two atoms - This increase the forces of attraction between the electrons and nuclei of the atoms - As a result of this, the atoms are pulled closer together causing a shorter bond length - The increased forces of attraction also means that the covalent bond is stronger

Answer 19

- The valence shell electron pair repulsion theory (VSEPR) predicts the shape and bond angles of molecules - Electrons are negatively charged and will repel other electrons when close to each other - In a molecule, the bonding pair of electrons will repel other electrons around the central atom forcing the molecule to adopt a shape in which these repulsive forces are minimised

Answer 20

- Valence shell electrons are those electrons that are found in the outer shell - Electron pairs repel each other as they have similar charges - Lone pair electrons repel each other more than bonded pairs - Repulsion between multiple and single bonds is treated the same as for repulsion between single bonds - Repulsion between pairs of double bonds are greater - The most stable shape is adopted to minimize the repulsion forces

Answer 21

- Lone pairs of electrons have a more concentrated electron charge cloud than bonding pairs of electrons - The cloud charges are wider and closer to the central atom’s nucleus - The order of repulsion is therefore: lone pair – lone pair > lone pair – bond pair > bond pair – bond pair

Answer 22

is the strongest form of intermolecular bonding - ---Intermolecular bonds are bonds between molecules - ---Hydrogen bonding is a type of permanent dipole – permanent dipole bonding - For hydrogen bonding to take place the following is needed: - ---A species which has an O or N (very electronegative) atom with an available lone pair of electrons - ---A species with an -OH or -NH group - When hydrogen is covalently bonded to an electronegative atom, such as O or N, the bond becomes very highly polarised - The H becomes so δ+ charged that it can form a bond with the lone pair of an O or N atom in another molecule -For hydrogen bonding to take place, the angle between the -OH/-NH and the hydrogen bond is 180o

Answer 23

- The number of hydrogen atoms attached to O or N in the molecule - The number of lone pairs on the O or N

Answer 24

-Hydrogen bonding in water, causes it to have anomalous properties such as high melting and boiling points, high surface tension and anomalous density of ice compared to water

Answer 25

- Water has high melting and boiling points which is caused by the strong intermolecular forces of hydrogen bonding between the molecules - In ice (solid H2O) and water (liquid H2O) the molecules are tightly held together by hydrogen bonds - A lot of energy is therefore required to break the water molecules apart and melt or boil them

Answer 26

- Water has a high surface tension - Surface tension is the ability of a liquid surface to resist any external forces (i.e. to stay unaffected by forces acting on the surface) - The water molecules at the surface of liquid are bonded to other water molecules through hydrogen bonds - These molecules pull downwards on the surface molecules causing the surface them to become compressed and more tightly together at the surface - This increases water’s surface tension All because of hydrogen bonding between water molecules

Answer 27

- Solids are denser than their liquids as the particles in solids are more closely packed together than in their liquid state - In ice however, the water molecules are packed in a 3D hydrogen-bonded network in a rigid lattice - Each oxygen atom is surrounded by hydrogen atoms - This way of packing the molecules in a solid and the relatively long bond lengths of the hydrogen bonds means that the water molecules are slightly further apart than in the liquid form - Therefore, ice has a lower density than liquid water

Answer 28

due to the increased number of electrons in the Group 16 elements - This causes an increased instantaneous dipole – induced dipole forces as the molecules become larger - Based on this, H2O would have a much lower enthalpy change (around 17 kJ mol-1) - However, the enthalpy change of vaporisation is almost 3 times larger which is caused by the hydrogen bonds present in water but not in the other hydrides

Answer 29

energy required to boil a substance

Answer 30

is the ability of an atom to draw a pair of electrons towards itself in a covalent bond -Electronegativity increases across a Period and decreases going down a Group

Answer 31

- When two atoms in a covalent bond have the same electronegativity the covalent bond is nonpolar - When two atoms in a covalent bond have different electronegativities the covalent bond is polar and the electrons will be drawn towards the more electronegative atom - As a result of this: - --The negative charge centre and positive charge centre do not coincide with each other - --This means that the electron distribution is asymmetric - --The less electronegative atom gets a partial charge of δ+ (delta positive) - --The more electronegative atom gets a partial charge of δ- (delta negative)

Answer 32

- The dipole moment is a measure of how polar a bond is - The direction of the dipole moment is shown by the following sign in which the arrow points to the partially negatively charged end of the dipole: -The sign shows the direction of the dipole moment and the arrow points to the delta negative end of the dipole

Answer 33

-To determine whether a molecule with more than two atoms is polar, the following things have to be taken into consideration: - --The polarity of each bond - --How the bonds are arranged in the molecule -Some molecules have polar bonds but are overall not polar because the polar bonds in the molecule are arranged in such way that the individual dipole moments cancel each other out

Answer 34

- Covalent bonds are strong intramolecular forces - Molecules also contain weaker intermolecular forces which are forces between molecules - These intermolecular forces are called van der Waals’ forces - There are two types of van der Waals’ forces: - ---Instantaneous (temporary) dipole – induced dipole forces also called London dispersion forces - ---Permanent dipole – permanent dipole forces

Answer 35

- Instantaneous dipole – induced dipole forces or London dispersion forces exist between all atoms or molecules - The electron charge cloud in non-polar molecules or atoms are constantly moving - During this movement, the electron charge cloud can be more on one side of the atom or molecule than the other - This causes a temporary dipole to arise - This temporary dipole can induce a dipole on neighbouring molecules - When this happens, the δ+ end of the dipole in one molecule and the δ- end of the dipole in a neighbouring molecule are attracted towards each other - Because the electron clouds are moving constantly, the dipoles are only temporary Weakest attraction London force is part of all bonding

Answer 36

- Hydrogen bonding is an intermolecular force between molecules with an -OH/-NH group and molecules with an N/O atom - Hydrogen bonding is a special case of a permanent dipole – dipole force between molecules - ---Hydrogen bonds are stronger forces than pd – pd forces - The hydrogen is bonded to an O/N atom which is so electronegative, that almost all the electron density from the covalent bond is drawn towards the O/N atom - This leaves the H with a large delta positive and the O/N with a large delta negative charging resulting in the formation of a permanent dipole in the molecule - A delta positive H in one molecule is electrostatically attracted to the delta negative O/N in a neighbouring molecule Strongest attraction

Answer 37

- Polar molecules have permanent dipoles - The molecule will always have a negatively and positively charged end - Forces between two molecules that have permanent dipoles are called permanent dipole – permanent dipole forces -The δ+ end of the dipole in one molecule and the δ- end of the dipole in a neighbouring molecule are attracted towards each other Medium strength Forms when two elements bond which have different electro-negativity

Answer 38

- --Butane and propanone have the same number of electrons - --Butane is a nonpolar molecule and will have id – id forces - --Propanone is a polar molecule and will have pd – pd forces - --Therefore, more energy is required to break the intermolecular forces between propanone molecules than between butane molecules So, propanone has a higher boiling point than butane

Answer 39

- Intramolecular forces are forces within a molecule - Ionic bonding is the electrostatic attraction between positive (cations) and negative (anions) ions in an ionic crystal lattice - ---These ions are formed by transferring the electrons from one species to the other - Covalent bonds are formed when the outer electrons of two atoms are shared - Metallic bonding is the electrostatic attraction of positively charged metal ions and their delocalised electrons in a metal lattice Form strong covalent bonds

Answer 40

-Intramolecular forces are forces between molecules and are also called van der Waals’s forces Intermolecular forces are responsible for melting and boiling point by of simple covalent bonds

Answer 41

stronger than intermolecular forces

Answer 42

- Metallic bonding - ionic bonding - covalent - hydrogen bonding - permanent dipole - permanent dipole forces - Instantaneous dipole - induced dipole

Answer 43

are diagrams that show the arrangement of the outer-shell electrons in an ionic or covalent compound or element The electrons are shown as dots and crosses

Answer 44

- --Only the outer electrons are shown - --The charge of the ion is spread evenly which is shown by using brackets - --The charge on each ion is written at the top right-hand corner

Answer 45

- Ionic bonds are formed when metal transfer electrons to a non-metal to form a positively charged and negatively charged ion - The atoms achieve a noble gas configuration

Answer 46

-Coordinate bonding or also called dative covalent bonding is formed when one atom provides both the electrons needed for a covalent bond - In a displayed formula, the dative covalent bond is represented by an arrow - The head of the arrow points away from the lone pair that forms the bond

Answer 47

Proportional to the change of ions Inversely proportional to the square of distance between ions E ∝ (Q^+) + (Q^-) // d^2 Attraction between cations and anions

Answer 48

Electrostatic force between neighbouring nuclei and shared electron No electron transfer but there is electron sharing

Answer 49

From period 3 onwards the d orbital can form part of the bonding with leads to more then 8 electrons in the outer most valance shell Why? Empty d orbital

Answer 50

1) size of molecules - size bigger = more electrons - easier to from a temporary dipole - more energy required to overcome L.F 2) contact point - greater contact points = higher London forces between the molecules

Answer 51

1) size of molecules - size bigger = more electrons - easier to from a temporary dipole - more energy required to overcome L.F 2) contact point - greater contact points = higher London forces between the molecules