Chemistry Chapter on Ionization Energy and Isotopes

False (B)

It decreases first ionisation energy.

<p>decreases, atomic radius, electron shielding</p> Signup and view all the answers

<p>Increasing nuclear charge = Increases first ionisation energy Increasing atomic radius = Decreases first ionisation energy Increasing electron shielding = Decreases first ionisation energy</p> Signup and view all the answers

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

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

<p>Magnesium has a larger atomic radius and increased electron shielding compared to beryllium.</p> Signup and view all the answers

<p>2 (B)</p> Signup and view all the answers

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

<p>1.1%</p> Signup and view all the answers

<p>48</p> Signup and view all the answers

<p>46Ti = 8.25% 47Ti = 7.44% 48Ti = 73.72% 49Ti = 5.41% 50Ti = 5.18%</p> Signup and view all the answers

<p>To identify the composition of stars (A)</p> Signup and view all the answers

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

<p>2 moles of hydrogen atoms or 4 hydrogen atoms total.</p> Signup and view all the answers

<p>2 (A)</p> Signup and view all the answers

<p>The molecule contains only carbon-12 and not carbon-13.</p> Signup and view all the answers

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

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

<p>SO2</p> Signup and view all the answers

<p>Ethene = CH2 Sulphuric Acid (H2SO4) = H2SO4 Magnesium Oxide = MgO Carbon Dioxide = CO2</p> Signup and view all the answers

<p>98 g/mol (C)</p> Signup and view all the answers

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

<p>Strong metallic bonds (A)</p> Signup and view all the answers

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

<p>metallic bonds</p> Signup and view all the answers

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

<p>High melting points = Strong attraction between metal ions and delocalised electrons Good electrical conductivity = Movement of delocalised electrons Strength = No individual bonds to break Bond strength = Depends on the charge and size of the ion</p> Signup and view all the answers

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

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

<p>Free moving electrons</p> Signup and view all the answers

<p>SnI4 (A)</p> Signup and view all the answers

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

<p>0.80 g</p> Signup and view all the answers

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

<p>Mass of the compound and mass of carbon (B)</p> Signup and view all the answers

<p>SnI4 = Tin and iodine SnCl2 = Tin and chlorine H2O = Hydrogen and oxygen C6H12O6 = Carbon, hydrogen, and oxygen</p> Signup and view all the answers

<p>65.2%</p> Signup and view all the answers

<p>189.2</p> Signup and view all the answers

<p>Actual Yield / Theoretical Yield x 100 (B)</p> Signup and view all the answers

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

<p>Sulfur dioxide and carbon dioxide</p> Signup and view all the answers

<p>percentage yield = (actual yield / theoretical yield) x 100</p> Signup and view all the answers

<p>Carbon Dioxide = Varies based on supplied reactants Sulfur Dioxide = Depends on actual yield of the reaction</p> Signup and view all the answers

<p>Incomplete reaction or loss during transfer (B)</p> Signup and view all the answers

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

<p>91.0%</p> Signup and view all the answers

Atoms with the same number of protons (atomic number) but different numbers of neutrons. This affects the mass.

A unique pattern of colors produced when an element is heated. It reveals the composition of a substance.

The average mass of a titanium atom, taking into account the percentages of different isotopes.

Different forms of the element Titanium with varying numbers of neutrons.

A technique used to identify and measure the relative abundance of isotopes by their mass/charge ratio

An isotope of carbon with 6 protons and 7 neutrons.

The weighted average mass of carbon atoms, considering abundances of carbon isotopes.

A peak in a mass spectrum representing a molecule with one isotope of a heavier mass

To find the number of hydrogen atoms in 16g of sulphuric acid (H2SO4), determine the moles of H2SO4 first, then multiply by the number of hydrogen atoms per molecule.

One mole of oxygen (O2) contains 1 * 6.02 x 10^23 oxygen molecules. Each oxygen molecule has 2 oxygen atoms.

The simplest whole-number ratio of elements in a compound.

Determine the elements' ratios to find the simplest formula that reflects the composition.

Empirical formula represents the simplest ratio, while the molecular formula shows the actual number of atoms of each element.

Convert percentages to grams, divide by molar mass to find moles of each element and then simplify the ratio of moles to the lowest whole number.

Calculate the molar ratios of each element, convert the percentages to grams, and express the ratios in the smallest whole numbers.

Mole is the amount of substance containing Avogadro's number of particles.

Increases across a period due to the increasing nuclear charge and decreasing atomic radius. This leads to greater attraction of electrons to the nucleus.

Decreases down a group due to increasing atomic radius and increased electron shielding. This weakens the attraction between the outer electrons and the nucleus.

Lithium will have a lower first ionization energy than carbon because of its smaller nuclear charge and larger atomic radius, resulting in less pull on the outer electrons.

Magnesium will have a lower first ionization energy than Beryllium because of its larger atomic radius and more shielding between outer electrons and the nucleus.

Increases the attraction between the positively charged nucleus and the negatively charged electrons, making it harder to remove an electron.

Decreases the attraction between the nucleus and the outer electrons, making it easier to remove an electron.

Reduces the attraction between the nucleus and outer electrons by creating a barrier between them.

The energy required to remove an electron from an atom in its gaseous state.

Strong electrostatic attraction between positive metal ions and a 'sea' of delocalized electrons.

A giant structure composed of metal ions surrounded by delocalized electrons.

Metals have high melting points due to strong metallic bonds holding the atoms together.

Metals conduct electricity because delocalized electrons can move freely.

Electrons that are not associated with a single atom but are free to move throughout the structure.

The greater the positive charge on the metal ion, the stronger the attraction, and therefore, the stronger the metallic bond.

Smaller ions lead to a stronger electrostatic attraction, making the metallic bond stronger.

A large arrangement of metal atoms held together by metallic bonding (a 'sea' of delocalized electrons).

The percentage by mass of each element in a compound. It represents the proportion of each element's mass relative to the total mass of the compound.

To calculate percentage composition, divide the mass (or atomic mass) of the element by the total mass (or molecular mass) of the compound and multiply by 100%.

The number of water molecules that are chemically bound to each formula unit of a salt in its crystalline form.

A salt that does not contain water molecules in its crystal structure.

To determine the number of water molecules in a hydrated salt, you can calculate the mass of water lost upon heating and use the molar masses to find the ratio of water molecules to salt molecules.

The formula of a hydrated salt includes the salt formula and a dot followed by the number of water molecules per formula unit (e.g., CuSO4.5H2O).

A process that involves the rearrangement of atoms and molecules, resulting in the formation of new substances.

A chemical equation where the number of atoms of each element is the same on both sides of the equation, ensuring the law of conservation of mass.

The ratio of the actual yield of a reaction to the theoretical yield, expressed as a percentage. It measures the efficiency of a chemical reaction.

The amount of product that is actually produced in a chemical reaction.

The maximum amount of product that can be produced from a given amount of reactants, based on the balanced chemical equation.

The formula used to calculate the percentage yield: (Actual Yield / Theoretical Yield) x 100%.

A chemical reaction where carbon disulfide reacts with oxygen to produce carbon dioxide and sulfur dioxide.

The study of the quantitative relationships between reactants and products in chemical reactions.

Converting moles of a substance to grams using its molar mass.