Atomic Theory and Structure Quiz

Atoms are tiny particles made of elements. Atoms cannot be divided. All the atoms in an element are the same. Atoms of one element are different to those of other elements.

Electrons have a negative charge. Electrons can be deflected by electromagnetic fields. Electrons have very small mass.

Protons and neutrons are found in the nucleus. Electrons orbit the nucleus in shells. The nucleus is tiny compared to the total volume of the atom. Most of the atom's mass is in the nucleus. Most of the atom is empty space between the nucleus and the electrons.

<p>Proton = +1, Electron = -1</p> Signup and view all the answers

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

<p>Protons and neutrons</p> Signup and view all the answers

<p>The atomic number is equal to the number of protons in an atom.</p> Signup and view all the answers

<p>Mass number = number of protons + number of neutrons</p> Signup and view all the answers

<p>Number of neutrons = mass number - atomic number</p> Signup and view all the answers

<p>Atoms of the same element with different numbers of neutrons and therefore different mass numbers.</p> Signup and view all the answers

<p>Neutrons have no impact on the chemical reactivity. Reactions involve electrons, isotopes have the same number of electrons in the same arrangement.</p> Signup and view all the answers

<p>The weighted mean mass of an atom of an element compared with one twelfth of the mass of an atom of carbon-12.</p> Signup and view all the answers

<p>Mass number</p> Signup and view all the answers

<p>Contribution of the electron is neglected. Mass of both proton and neutron is taken as 1.0 u.</p> Signup and view all the answers

<p>Both can be calculated by adding the relative atomic masses of each of the atoms making up the molecule or the formula.</p> Signup and view all the answers

<p>Identify unknown compounds. Find relative abundance of each isotope of an element. Determine structural information.</p> Signup and view all the answers

<p>The m/z value of the M+ ion is the value of the last peak - 72</p> Signup and view all the answers

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

<p>(124 x 2) + (126 x 4) + (128 x 7) + (130 x 6) or 2428/19 or 127.8 or (124 x 10.5) + (126 x 21.1) + (128 x 36.8) + (130 x 31.6) or 2428/19 or 127.8</p> Signup and view all the answers

<p>The shell occupied by the electrons.</p> Signup and view all the answers

<p>A group of orbitals with the same principal quantum number.</p> Signup and view all the answers

<p>2</p> Signup and view all the answers

<p>A region around the nucleus that can hold up to two electrons with opposite spins</p> Signup and view all the answers

<p>2</p> Signup and view all the answers

<p>s orbital, p orbital, d orbital, f orbital</p> Signup and view all the answers

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

<p>1</p> Signup and view all the answers

<p>2</p> Signup and view all the answers

<p>3</p> Signup and view all the answers

<p>5</p> Signup and view all the answers

<p>14</p> Signup and view all the answers

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

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

<p>n = 1</p> Signup and view all the answers

<p>Electrons are added one at a time. Lowest available energy level is filled first. Each energy level must be filled before the next one can fill. Each orbital is filled singly before pairing. 4s is filled before 3d.</p> Signup and view all the answers

<p>The 4s orbital has a lower energy than the 3d orbital before it is filled.</p> Signup and view all the answers

<p>1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6</p> Signup and view all the answers

<p>The noble gas before the element is used to abbreviate. E.g Li → 1s22s1 ; Li → [He] 2s1</p> Signup and view all the answers

<p>They are arranged in the order of increasing atomic numbers.</p> Signup and view all the answers

<p>The group number is equal to the number of electrons in the outer shell.</p> Signup and view all the answers

<p>The horizontal rows.</p> Signup and view all the answers

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

<p>The repeating trends in chemical and physical properties.</p> Signup and view all the answers

<p>Elements change from metals to non-metals.</p> Signup and view all the answers

<p>The energy required to remove a mole of electrons from a mole of gaseous atoms to form one mole of gaseous 1+ ions under standard conditions.</p> Signup and view all the answers

<p>Mg(g) → Mg+(g) + e-</p> Signup and view all the answers

<p>Atomic radius, Nuclear charge, Electron shielding or screening</p> Signup and view all the answers

<p>First Ionisation energy increases across a period because of: Increased nuclear charge. Decreased atomic radius. Same electron shielding. This means more energy is needed to remove the first electron. Dips at Al because: outer electron is in a 3p orbital, higher energy than 3s orbital → less energy needed to remove electron. Dips at S because one 3p orbital contains two electrons → repulsion between paired electrons → less energy needed to remove one.</p> Signup and view all the answers

<p>Decreases between 2 to 3 because in group 3 the outermost electrons are in p orbitals. Whereas in group 2 they are in s orbital, so the electrons are easier to be removed.</p> Signup and view all the answers

<p>Decrease. There is an increase in atomic radius. Increase in electron shielding.</p> Signup and view all the answers

<p>Decrease. Shielding increases → weaker attraction. Atomic radius increases → distance between the outer electrons and nucleus increases → weaker attraction. Increase in number of protons is outweighed by increase in distance and shielding.</p> Signup and view all the answers

<p>Li &amp; Be → giant metallic ; strong attraction between positive ions and delocalised electrons ; metallic bonding. B &amp; C → giant covalent ; strong forces between atoms ; covalent. N2, O2, F2, Ne → simple molecular ; weak intermolecular forces between molecules ; covalent bonding within molecules and intermolecular forces between molecules.</p> Signup and view all the answers

Atoms are tiny particles, indivisible, and identical within elements.

Electrons have a negative charge, can be deflected, and are very light.

Nucleus contains protons and neutrons; electrons orbit in shells.

Proton = +1 charge; Electron = -1 charge.

Neutrons and protons have roughly the same mass.

Most mass comes from protons and neutrons.

Determines the number of protons in an atom.

Mass number = number of protons + neutrons.

Calculate neutrons: Neutrons = mass number - atomic number.

Atoms of the same element with differing neutron numbers.

Different isotopes react similarly due to same electron arrangement.

Weighted average mass of an element’s atoms compared to carbon-12.

Mass of a specific isotope relative to carbon-12.

Relative isotopic mass equals the mass number of an isotope.

Neglect electron mass; consider protons and neutrons as 1.0 u each.

Sum of relative atomic masses of all atoms in the molecule.

Identify compounds, measure isotope abundance, and understand structures.

Indicates the electron shell occupied by electrons.

Groups of orbitals with the same principal quantum number.

The first shell can hold 2 electrons.

The second shell can hold 8 electrons.

The third shell can hold 18 electrons.

Region where up to two electrons with opposite spins can exist.

s, p, d, and f orbitals, each with distinct shapes.

Using the last noble gas to simplify electron configuration.

Elements arranged by increasing atomic number and grouped by properties.

Group number indicates the number of outer shell electrons.