Chemistry Atomic Structure Trends

False (B)

It indicates the presence of carbon-13 isotopes in the organic compound.

<p>the compound</p> Signup and view all the answers

<p>Cl = Has two isotopes, 35Cl and 37Cl Ag = Forms insoluble compounds with halides K = Forms soluble salts with nitrates Ba = Has limited solubility in sulfates</p> Signup and view all the answers

<p>AgCl forms as a solid (C)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>A strong electrostatic attraction between positive and negative ions.</p> Signup and view all the answers

<p>Blue (B)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>Dative covalent bond (B)</p> Signup and view all the answers

<p>The layers may slide over each other.</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>polarizing power</p> Signup and view all the answers

<p>Polarizing power = Ability of a positive ion to distort a negative ion's electron cloud Polarisability = Ability of a negative ion to be distorted by a positive ion Expanded octet = The availability of d-subshell to accommodate extra electrons Simple molecule = Low melting and boiling points due to weak intermolecular forces</p> Signup and view all the answers

<p>C2H5Cl</p> Signup and view all the answers

<p>uncharged</p> Signup and view all the answers

<p>Higher charge (C)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>Molecular Formula = Actual number of each atom in a molecule Empirical Formula = Simplest whole number ratio of atoms Structural Formula = Describes how atoms are joined together Displayed Formula = Shows every atom and bond in a molecule</p> Signup and view all the answers

<p>Strong electrostatic attraction between oppositely charged ions in a giant lattice.</p> Signup and view all the answers

<p>Each bonding electron leaves with different atoms (D)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>The yield is low due to further substitution reactions and separation of products.</p> Signup and view all the answers

<p>It increases (B)</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>A region within an atom that can hold up to two electrons with opposing spins.</p> Signup and view all the answers

<p>gaseous ions</p> Signup and view all the answers

<p>29Cu = 1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d10 24Cr = 1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d Hydrogen = 1s1 Oxygen = 1s2, 2s2, 2p4</p> Signup and view all the answers

<p>Increased atomic radius (C)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>Nuclear charge, distance of outer electrons from the nucleus, shielding effect of inner electrons, spin-pair repulsion.</p> Signup and view all the answers

<p>C=C double bond (A)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>Electrophilic addition</p> Signup and view all the answers

<p>combination</p> Signup and view all the answers

<p>Graphite = Conducts electricity Diamond = High melting point Benzene = Aromatic compound Carbon Black = Used in tires</p> Signup and view all the answers

<p>Polymers need to be sorted and this is expensive. (D)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>Reduced electron-electron repulsion</p> Signup and view all the answers

<p>beryllium</p> Signup and view all the answers

<p>Delocalized electrons (B)</p> Signup and view all the answers

Atomic radius decreases across a period because the increasing nuclear charge (more protons) attracts the outer electrons more strongly, despite them being in the same shell.

Atomic radius increases down a group because the outer electrons are further from the nucleus due to additional electron shells, reducing the attraction.

A region within an atom that can hold up to two electrons with opposing spins.

The energy required to remove one mole of electrons from one mole of gaseous atoms to form gaseous ions. It's an endothermic process.

The larger the nuclear charge, the stronger the attraction between the nucleus and outer electrons, making it harder to remove.

The closer an electron is to the nucleus, the stronger the attraction, and the more difficult it is to remove.

Inner electron shells shield outer electrons from the nucleus, reducing the attraction and making it easier to remove them.

Two electrons in the same orbital repel each other, making it easier to remove one of them.

The tendency of an atom's outermost electron to be attracted to the nucleus, increasing across a period.

The difference in the attraction between the nucleus and the outermost electron due to inner electrons shielding the outer electron from the nucleus's pull. This is almost constant across a period.

The process in mass spectrometry where the sample is heated to transform it into a gas.

The process in mass spectrometry where the sample is bombarded with high-speed electrons, causing the sample to lose electrons and become ions.

The process in mass spectrometry where ions are accelerated by a negatively charged plate in a vacuum.

The process in mass spectrometry where ions are deflected by a magnetic field. The amount of deflection is dependent on the mass-to-charge ratio (m/z).

The strongest peak in the mass spectrum representing the molecule with the highest mass-to-charge ratio (m/z).

A small peak next to the M+ peak in the mass spectrum due to the presence of the carbon-13 isotope. The height of the M+1 peak is directly proportional to the number of carbon atoms in the compound.

The electrostatic attraction force between oppositely charged ions in a giant three-dimensional lattice structure.

Ionic compounds conduct electricity when molten or dissolved in water because the ions become free to move and carry charge.

Ionic compounds are brittle due to the strong electrostatic forces holding them together. If one layer shifts slightly, same-charged ions repel, causing fracture.

The ability of a positive ion (cation) to distort the electron cloud of a neighboring negative ion (anion).

The measure of how easily the electron cloud of a negative ion (anion) can be distorted by a positive ion (cation).

The electrostatic attraction force between two bonded atoms, arising from the shared pair of electrons between them.

Elements with an expanded octet can accommodate more than eight electrons in their outer shell by using their vacant d-orbitals.

Simple molecules have weak intermolecular forces, which require a small amount of energy to overcome, resulting in low melting and boiling points.

A bond formed when one atom donates a pair of electrons to another atom, which has an empty orbital.

The representation of a molecule that shows the arrangement of atoms and how they are connected.

The simplest whole number ratio of atoms in a compound.

The breaking of a covalent bond where both bonding electrons are taken by one atom, forming a negative ion and leaving the other atom as a positive ion.

The breaking of a covalent bond where each bonding electron leaves with one species, forming a free radical.

A species that contains an unpaired electron and is uncharged.

Isomerism that arises due to different spatial arrangements of atoms around a double bond.

A molecule with an uneven distribution of electron density, resulting in a separation of charge.

The restricted rotation around the double bond in alkenes is due to the presence of a pi bond, which is a region of high electron density.

Polymers are large molecules formed by the joining of many smaller repeating units called monomers.

Alkenes are attracted to electrophiles because the pi bond creates a region of high electron density.

An electrophile is a molecule that seeks out regions of high electron density. In electrophilic addition reactions, an electrophile attacks a molecule with high electron density, resulting in the formation of a single product.

Secondary carbocations are more stable than primary carbocations because they have more electron-donating alkyl groups, which stabilize the positive charge.

Boron has a lower first ionization energy than beryllium because the 2p electron being removed in boron is further from the nucleus and more shielded by the 2s electrons.

Graphite and diamond are giant covalent structures with strong covalent bonds between the atoms. They are held together by these strong bonds, which require a lot of energy to break.

Sulfur has a lower first ionization energy because one of its 3p orbitals is doubly filled, leading to electron repulsion between the electrons in the same orbital, making it easier to remove one of them.

Incineration reduces landfill volume and generates energy, but it also produces toxins. Recycling saves resources but requires sorting and energy.

The bond angle in ammonia (NH3) is approximately 107 degrees because the lone pair on the nitrogen atom repels the bonding pairs more strongly, pushing them closer together.