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identity."},{"text":"Smallest particle of a compound that can take part in chemical reactions.","correct":false,"explanation":"A molecule is made from two or more chemically bonded atoms, so it is not the definition of an atom. The correct answer describes the smallest reactive particle of an element."},{"text":"Smallest particle of an ion that can take part in chemical reactions.","correct":false,"explanation":"An ion is a charged atom or group of atoms formed by electron loss or gain. The correct definition focuses on the smallest reactive particle of an element."},{"text":"Smallest particle of a mixture that can take part in chemical reactions.","correct":false,"explanation":"An element is a substance containing one type of atom, not a single particle defined by chemical reactions. The correct answer identifies the smallest particle of an element."}]},{"id":"8df29b18-65c8-498c-b389-e62258903a26","cardType":"cloze","points":null,"front":"A [ ] is a group of two or more atoms chemically bonded together.","back":"A molecule is a group of two or more atoms chemically bonded together.","mcqOptions":[{"text":"molecule","correct":true,"explanation":"A molecule consists of two or more atoms joined by chemical bonds, whether the atoms are from the same element or from different elements."},{"text":"element","correct":false,"explanation":"An element contains only one type of atom and is not defined by the number of atoms chemically bonded together. The correct term for such a group is molecule."},{"text":"compound","correct":false,"explanation":"A compound contains atoms of at least two different elements chemically combined. The sentence describes any bonded group of two or more atoms, which is a molecule."},{"text":"ion","correct":false,"explanation":"An ion is a charged atom or group of atoms, whereas the sentence describes a group specifically by chemical bonding. The correct term is molecule."}]},{"id":"951787d4-9e8a-41df-bcff-146341e8f19d","cardType":"basic","points":2,"front":"Why is $O_2$ a molecule but NOT a compound?","back":"It contains two atoms bonded together, but only one type of element.","mcqOptions":[{"text":"It contains two atoms bonded together, but only one type of element.","correct":true,"explanation":"Oxygen gas contains two oxygen atoms bonded together, but both atoms belong to the same element. A compound must contain two or more different elements."},{"text":"It contains two atoms bonded together, and two types of element.","correct":false,"explanation":"Having two different types of element would make the substance a compound. In oxygen gas, both bonded atoms are oxygen, so it contains one type of element."},{"text":"It contains two atoms separate from each other, but only one type of element.","correct":false,"explanation":"The atoms in oxygen gas are chemically bonded, so describing them as separate is incorrect. It contains two atoms bonded together, but only one type of element."},{"text":"It contains one atom bonded together, but only two types of element.","correct":false,"explanation":"A compound requires different elements, but oxygen gas contains identical oxygen atoms. The number of bonded atoms is two, while the number of element types is one."}]},{"id":"59629a8b-80d4-4b35-b502-8321f234aff0","cardType":"basic","points":3,"front":"State the location, relative mass, and relative charge of a proton.","back":"

Location: nucleus
Relative mass: 1
Relative charge: +1

","mcqOptions":[{"text":"

Location: nucleus
Relative mass: 1
Relative charge: +1

","correct":true,"explanation":"Protons are found in the nucleus, have a relative mass of 1, and carry one positive unit of charge."},{"text":"

Location: nucleus
Relative mass: 1
Relative charge: 0

","correct":false,"explanation":"This combines the proton’s location and mass with the neutron’s charge. The correct proton values are nucleus, relative mass 1, and relative charge +1."},{"text":"

Location: shells (around nucleus)
Relative mass: 1/1836 (nearly 0)
Relative charge: -1

","correct":false,"explanation":"Electrons occupy shells, have very little relative mass, and are negatively charged. The correct proton values are nucleus, relative mass 1, and relative charge +1."},{"text":"

Location: shells (around nucleus)
Relative mass: 1
Relative charge: +1

","correct":false,"explanation":"A proton is not found in shells and does not have negligible mass. Those properties belong to an electron; the correct proton values are nucleus, 1, and +1."}]},{"id":"081bc9b5-9e65-4cf5-9fb9-bab3c07aa2b4","cardType":"basic","points":3,"front":"State the location, relative mass, and relative charge of a neutron.","back":"

Location: nucleus
Relative mass: 1
Relative charge: 0

","mcqOptions":[{"text":"

Location: nucleus
Relative mass: 1
Relative charge: 0

","correct":true,"explanation":"Neutrons are located in the nucleus, have a relative mass of 1, and have no charge, unlike positively charged protons and negatively charged electrons."},{"text":"

Location: shells (around nucleus)
Relative mass: 1/1836 (nearly 0)
Relative charge: 0

","correct":false,"explanation":"A zero charge identifies a neutron, but electrons are found in shells and have very little mass. The correct neutron values are nucleus, relative mass 1, and charge 0."},{"text":"

Location: nucleus
Relative mass: 1
Relative charge: +1

","correct":false,"explanation":"A positive charge identifies a proton, not a neutron. The correct neutron is in the nucleus, has relative mass 1, and has relative charge 0."},{"text":"

Location: shells (around nucleus)
Relative mass: 1
Relative charge: -1

","correct":false,"explanation":"Neutrons are not negatively charged or located in shells. Those are electron properties; the correct values for a neutron are nucleus, relative mass 1, and charge 0."}]},{"id":"ec259304-e15a-47fc-af57-6024932c6122","cardType":"basic","points":3,"front":"State the location, relative mass, and relative charge of an electron.","back":"

Location: shells (around nucleus)
Relative mass: 1/1836 (nearly 0)
Relative charge: -1

","mcqOptions":[{"text":"

Location: shells (around nucleus)
Relative mass: 1/1836 (nearly 0)
Relative charge: -1

","correct":true,"explanation":"Electrons occupy shells around the nucleus, have a relative mass of 1/1836, which is nearly zero, and carry one negative unit of charge."},{"text":"

Location: nucleus
Relative mass: 1
Relative charge: -1

","correct":false,"explanation":"Relative mass 1 and location in the nucleus describe protons and neutrons, not electrons. The correct electron values are shells, 1/1836, and -1."},{"text":"

Location: shells (around nucleus)
Relative mass: 1/1836 (nearly 0)
Relative charge: +1

","correct":false,"explanation":"The positive charge belongs to a proton. Electrons are negatively charged and have very little mass, so their correct values are shells, 1/1836, and -1."},{"text":"

Location: shells (around nucleus)
Relative mass: 1
Relative charge: -1

","correct":false,"explanation":"Electrons have negligible relative mass, not the mass of a proton or neutron. They are in shells and have charge -1; the correct relative mass is 1/1836."}]},{"id":"ff3d21c7-a733-4275-a9e6-04cff62a9a79","cardType":"basic","points":1,"front":"Why are atoms electrically neutral?","back":"They have the same number of positive protons and negative electrons.","mcqOptions":[{"text":"They have the same number of positive protons and negative electrons.","correct":true,"explanation":"Atoms are neutral when the number of positively charged protons equals the number of negatively charged electrons, so the charges cancel overall."},{"text":"They have the same number of neutrons and negative electrons.","correct":false,"explanation":"Neutrons have no charge, so their number does not determine whether an atom is neutral. Neutrality requires the same number of positive protons and negative electrons."},{"text":"They have the same charge of positive protons and negative electrons.","correct":false,"explanation":"Protons and electrons have opposite charges, not the same charge. An atom is neutral when it has the same number of positive protons and negative electrons."},{"text":"They have the same number of positive protons and neutral neutrons.","correct":false,"explanation":"Equal numbers of protons and neutrons do not cancel charge because neutrons are neutral. The required balance is the same number of positive protons and negative electrons."}]},{"id":"1e2b735b-df15-4838-9b20-3b1a29b29323","cardType":"cloze","points":null,"front":"The [ ] contains most of the atom's mass because it holds the heavy protons and neutrons.","back":"The nucleus contains most of the atom's mass because it holds the heavy protons and neutrons.","mcqOptions":[{"text":"nucleus","correct":true,"explanation":"The nucleus contains protons and neutrons, each with a relative mass of about 1, while electrons have negligible mass and occupy shells around it."},{"text":"shells","correct":false,"explanation":"Shells contain the electrons, whose relative mass is nearly zero. Most of an atom’s mass is concentrated in the nucleus, containing its protons and neutrons."},{"text":"electron","correct":false,"explanation":"An electron is a single negatively charged particle with negligible relative mass, not the central region holding the heavy particles. The correct term is nucleus."},{"text":"proton","correct":false,"explanation":"A proton is a heavy particle within the central region, but it is not the whole region containing most atomic mass. That region is the nucleus."}]},{"id":"e19056d9-a481-4e4c-ac81-703084db25ab","cardType":"basic","points":1,"front":"What does the atomic number ($Z$) represent?","back":"The number of protons in the nucleus.","mcqOptions":[{"text":"The number of protons in the nucleus.","correct":true,"explanation":"The atomic number is defined as the number of protons in an atom’s nucleus. This value identifies the element because every element has a unique proton number."},{"text":"The number of neutrons in the nucleus.","correct":false,"explanation":"Neutron number can vary between isotopes, so it cannot identify the element. The atomic number is the number of protons in the nucleus."},{"text":"The total number of protons and neutrons in the nucleus.","correct":false,"explanation":"This describes the mass number, not the atomic number. The atomic number counts only the protons in the nucleus."},{"text":"The number of electrons in the outer shell.","correct":false,"explanation":"Electrons determine bonding and chemical behaviour, but their number can change when ions form. The atomic number is the number of protons in the nucleus."}]},{"id":"38ad0684-bc4b-45b8-9d29-e784ce64a536","cardType":"basic","points":1,"front":"What does the mass number ($A$) represent?","back":"The total number of protons and neutrons in the nucleus.","mcqOptions":[{"text":"The total number of protons and neutrons in the nucleus.","correct":true,"explanation":"The mass number is the total number of nucleons, meaning protons plus neutrons, in the nucleus. Electrons have negligible mass and are not included."},{"text":"The number of protons in the nucleus.","correct":false,"explanation":"Counting only protons gives the atomic number, not the mass number. The mass number includes both protons and neutrons in the nucleus."},{"text":"The total number of protons and electrons in the atom.","correct":false,"explanation":"Electrons are not counted in the mass number because their masses are negligible. The mass number is found by adding protons and neutrons."},{"text":"The number of neutrons in the nucleus.","correct":false,"explanation":"The neutron count alone is not the mass number and changes between isotopes. The mass number is the combined total of protons and neutrons."}]},{"id":"a28893e6-9a24-4e5a-91ac-8dbca377a0f9","cardType":"basic","points":1,"front":"How is the number of neutrons calculated using $A$ and $Z$?","back":"$$$\\text{number of neutrons} = A - Z$$","mcqOptions":[{"text":"$$$\\text{number of neutrons} = A - Z$$","correct":true,"explanation":"The mass number, A, equals protons plus neutrons, while the atomic number, Z, equals protons. Subtracting Z from A therefore leaves the number of neutrons."},{"text":"$$$\\text{number of neutrons} = A + Z$$","correct":false,"explanation":"Adding A and Z counts the proton number twice rather than removing it. The correct calculation is A - Z because mass number includes protons and neutrons."},{"text":"$$$\\text{number of neutrons} = Z - A$$","correct":false,"explanation":"The atomic number is smaller than the mass number for ordinary atoms, so this reversal would produce a negative neutron count. Neutrons are calculated using A - Z."},{"text":"$$$\\text{number of neutrons} = A \\div Z$$","correct":false,"explanation":"Dividing the two numbers has no basis in the definitions of mass number and atomic number. Subtracting Z, the proton count, from A gives the neutron count."}]},{"id":"a7a74aed-8be8-4fef-b023-2c2fee68a3a9","cardType":"cloze","points":null,"front":"The [ ] identifies the element; if this number changes, it becomes a different element.","back":"The atomic number identifies the element; if this number changes, it becomes a different element.","mcqOptions":[{"text":"atomic number","correct":true,"explanation":"The atomic number identifies an element because it equals the number of protons. Changing the proton number changes the identity of the element."},{"text":"mass number","correct":false,"explanation":"The mass number can change when isotopes have different neutron numbers without changing the element. The atomic number identifies the element."},{"text":"number of neutrons","correct":false,"explanation":"Different isotopes of one element can have different neutron numbers, so this value does not determine identity. The atomic number does."},{"text":"number of electrons","correct":false,"explanation":"Atoms can gain or lose electrons to form ions while remaining the same element. Element identity is fixed by the atomic number."}]},{"id":"94f8bb98-c705-4807-8e34-0b763b1c1692","cardType":"basic","points":2,"front":"Define isotopes.","back":"Atoms of the same element with the same number of protons but different numbers of neutrons.","mcqOptions":[{"text":"Atoms of the same element with the same number of protons but different numbers of neutrons.","correct":true,"explanation":"Isotopes are atoms of the same element, so they have the same proton number, but they differ in neutron number, giving them different mass numbers."},{"text":"Atoms of different elements with the same number of protons but different numbers of neutrons.","correct":false,"explanation":"Different elements cannot have the same proton number, because proton number defines element identity. Isotopes are atoms of the same element with different neutron numbers."},{"text":"Atoms of the same element with different numbers of protons but the same number of neutrons.","correct":false,"explanation":"Changing the proton number changes the element itself, not just its isotope. Isotopes retain the same proton number and differ in neutron number."},{"text":"Atoms of the same element with the same number of neutrons but different numbers of electrons.","correct":false,"explanation":"Different electron numbers describe ions, not isotopes. Isotopes have the same proton number but different numbers of neutrons."}]},{"id":"44c5f713-b43e-49e0-8d9b-fbfc3d3ced91","cardType":"cloze","points":null,"front":"Isotopes of the same element have very similar [ ] because they have the same number of electrons.","back":"Isotopes of the same element have very similar chemical properties because they have the same number of electrons.","mcqOptions":[{"text":"chemical properties","correct":true,"explanation":"Chemical properties depend mainly on electron arrangement. Isotopes of an element have the same number of electrons in neutral atoms, so their chemical properties are very similar."},{"text":"physical properties","correct":false,"explanation":"Isotopes can have noticeably different physical properties, such as mass and some physical constants. Their similar behaviour mainly concerns chemical properties."},{"text":"mass numbers","correct":false,"explanation":"Isotopes have different mass numbers because they contain different numbers of neutrons. Their similar chemical properties result from their matching electron arrangements."},{"text":"nuclear properties","correct":false,"explanation":"Nuclear properties can differ substantially between isotopes, including radioactive stability. The shared electron arrangement makes their chemical properties very similar."}]},{"id":"2a0c975f-b6c0-4929-8884-d259f6752262","cardType":"cloze","points":null,"front":"Isotopes of the same element have very similar chemical properties because they have the same number of [ ].","back":"Isotopes of the same element have very similar chemical properties because they have the same number of electrons.","mcqOptions":[{"text":"electrons","correct":true,"explanation":"Neutral isotopes of the same element have the same proton number and therefore the same number of electrons. Their identical electron arrangements produce similar chemical properties."},{"text":"neutrons","correct":false,"explanation":"Isotopes differ specifically in their numbers of neutrons, so this cannot explain their similar chemical behaviour. The relevant shared particles are electrons."},{"text":"protons","correct":false,"explanation":"Isotopes do share the same number of protons, but chemical properties are governed mainly by electron arrangement. The blank refers to electrons."},{"text":"nucleons","correct":false,"explanation":"Nucleons include both protons and neutrons, and isotopes do not have the same total number of nucleons. Their chemical similarity comes from equal electron numbers."}]},{"id":"d6bacb06-ee9b-4257-bf82-5076c3e3b255","cardType":"basic","points":2,"front":"Why is the relative atomic mass ($A_r$) of many elements not a whole number?","back":"It is a weighted average of the masses of different isotopes.","mcqOptions":[{"text":"It is a weighted average of the masses of different isotopes.","correct":true,"explanation":"Relative atomic mass accounts for the masses of an element’s isotopes and their natural abundances. Weighting the isotope masses usually produces a non-whole-number average."},{"text":"It is the mass number of the most common isotope.","correct":false,"explanation":"Using only the most abundant isotope ignores the contributions of the other isotopes. Relative atomic mass is a weighted average based on all naturally occurring isotopes."},{"text":"It is the average number of protons and electrons in the atom.","correct":false,"explanation":"Relative atomic mass concerns isotope masses, not a count of protons and electrons. The electron contribution is negligible, and isotope abundances must be included."},{"text":"It is the total number of protons and neutrons in one atom.","correct":false,"explanation":"That total is the mass number for a particular isotope and is always a whole number. Relative atomic mass averages the masses of different isotopes."}]},{"id":"e481b086-d76b-4cf9-9cb4-3dc081cc2f53","cardType":"cloze","points":null,"front":"Relative atomic mass ($A_r$) is the [ ] of an atom compared to 1/12 of the mass of a carbon-12 atom.","back":"Relative atomic mass ($A_r$) is the weighted mean mass of an atom compared to 1/12 of the mass of a carbon-12 atom.","mcqOptions":[{"text":"weighted mean mass","correct":true,"explanation":"Isotopes contribute according to their natural abundances, so the relative atomic mass is the weighted mean of their individual isotopic masses."},{"text":"unweighted mean mass","correct":false,"explanation":"An unweighted mean treats every isotope as equally abundant. The correct term is weighted mean mass because more abundant isotopes contribute more to relative atomic mass."},{"text":"mass number","correct":false,"explanation":"Mass number is the total number of protons and neutrons in one particular atom. Relative atomic mass instead uses the weighted mean mass of all naturally occurring isotopes."},{"text":"proton number","correct":false,"explanation":"Proton number identifies an element and does not account for isotope masses or abundances. The required quantity is the weighted mean mass of the element’s isotopes."}]},{"id":"0888246c-cfd5-462b-b208-0c2aea46ff87","cardType":"cloze","points":null,"front":"Relative atomic mass ($A_r$) is the weighted mean mass of an atom compared to [ ] of the mass of a carbon-12 atom.","back":"Relative atomic mass ($A_r$) is the weighted mean mass of an atom compared to 1/12 of the mass of a carbon-12 atom.","mcqOptions":[{"text":"1/12","correct":true,"explanation":"The atomic mass unit is defined using exactly one-twelfth of the mass of a carbon-12 atom, providing the standard reference for relative atomic masses."},{"text":"1/6","correct":false,"explanation":"Using one-sixth would make the reference unit twice as large as defined. Relative atomic mass is compared with 1/12 of a carbon-12 atom’s mass."},{"text":"1/14","correct":false,"explanation":"The denominator does not come from the isotope carbon-14. The agreed standard is 1/12 of the mass of a carbon-12 atom."},{"text":"1/2","correct":false,"explanation":"Using half of a carbon-12 atom’s mass confuses the reference with six atomic mass units. The defined comparison is with 1/12 of its mass."}]},{"id":"8baa5883-36aa-4cc1-8009-d3d4bc796fc4","cardType":"basic","points":1,"front":"State the formula for $A_r$ using percentage abundances.","back":"$$$A_r = \\frac{\\text{∑(isotope mass % % abundance)}}{100}$$","mcqOptions":[{"text":"$$$A_r = \\frac{\\text{∑(isotope mass % % abundance)}}{100}$$","correct":true,"explanation":"Each isotope’s mass is multiplied by its percentage abundance, the products are summed, and division by 100 converts the percentages into proportions."},{"text":"$$$A_r = \\frac{\\text{∑(isotope mass % % abundance)}}{12}$$","correct":false,"explanation":"Dividing by 12 confuses the carbon-12 reference standard with the abundance calculation. Percentage-weighted products must be divided by 100."},{"text":"$$$A_r = \\frac{\\text{∑(isotope mass + % abundance)}}{100}$$","correct":false,"explanation":"Adding mass to percentage abundance mixes unlike quantities and does not produce a weighted mean. Each mass must be multiplied by its percentage abundance before dividing by 100."},{"text":"$$$A_r = \\frac{\\text{∑(isotope mass % % abundance)}}{\\text{number of isotopes}}$$","correct":false,"explanation":"Dividing by the number of isotopes incorrectly gives each isotope equal influence. With percentage abundances, the weighted sum must be divided by 100."}]},{"id":"0e192957-f64c-4cd8-8ec7-2b984887aed3","cardType":"basic","points":2,"front":"How is $A_r$ calculated if abundances are given as a ratio?","back":"Multiply mass by relative abundance, sum them, and divide by the total number of ratio parts.","mcqOptions":[{"text":"Multiply mass by relative abundance, sum them, and divide by the total number of ratio parts.","correct":true,"explanation":"Ratio abundances represent relative numbers of atoms, so each mass is weighted by its ratio value and the sum is divided by the total ratio parts."},{"text":"Multiply mass by relative abundance, sum them, and divide by the total number of isotopes.","correct":false,"explanation":"Dividing by the number of isotopes treats all isotopes as equally abundant, ignoring unequal ratio values. The denominator must be the total number of ratio parts."},{"text":"Multiply mass by relative abundance, sum them, and divide by 100.","correct":false,"explanation":"Division by 100 applies only when abundances are percentages. For ratio abundances, the weighted sum is divided by the total number of ratio parts."},{"text":"Multiply mass by relative abundance, sum them, and divide by the largest ratio part.","correct":false,"explanation":"The largest ratio value is not the total population represented by the ratio. The weighted sum must be divided by the sum of all ratio parts."}]},{"id":"b82c14ca-0b42-4153-bd7b-7a078f91bc85","cardType":"basic","points":2,"front":"An atom has atomic number 11 and mass number 23. Calculate the number of protons, neutrons, and electrons.","back":"

Protons: 11
Neutrons: 12 ($23 - 11$)
Electrons: 11

","mcqOptions":[{"text":"

Protons: 11
Neutrons: 12 ($23 - 11$)
Electrons: 11

","correct":true,"explanation":"Atomic number gives 11 protons, and a neutral atom also has 11 electrons. Subtracting atomic number from mass number gives 12 neutrons."},{"text":"

Protons: 11
Neutrons: 23 ($23$)
Electrons: 11

","correct":false,"explanation":"Using the mass number directly as the neutron count forgets that it includes both protons and neutrons. The correct counts are 11 protons, 12 neutrons, and 11 electrons."},{"text":"

Protons: 11
Neutrons: 12 ($23 - 11$)
Electrons: 12

","correct":false,"explanation":"The neutron calculation is correct, but a neutral atom’s electron count equals its proton count, not its neutron count. It therefore has 11 electrons."},{"text":"

Protons: 23
Neutrons: 12 ($23 - 11$)
Electrons: 23

","correct":false,"explanation":"Mass number is not the number of protons or electrons; atomic number supplies both counts in a neutral atom. The correct values are 11, 12, and 11."}]},{"id":"a588d22c-e152-4678-9ecb-064f3fc545ec","cardType":"basic","points":2,"front":"Compare the sub-atomic composition of Carbon-12 and Carbon-14.","back":"

Both have 6 protons.
Carbon-12 has 6 neutrons; Carbon-14 has 8 neutrons.

","mcqOptions":[{"text":"

Both have 6 protons.
Carbon-12 has 6 neutrons; Carbon-14 has 8 neutrons.

","correct":true,"explanation":"Both atoms are carbon because each has atomic number 6 and therefore six protons. Their mass-number difference results from carbon-14 having two additional neutrons."},{"text":"

Both have 12 protons.
Carbon-12 has 6 neutrons; Carbon-14 has 8 neutrons.

","correct":false,"explanation":"The 12 in carbon-12 is its mass number, not its proton number. Both isotopes have 6 protons, while their neutron counts are 6 and 8."},{"text":"

Both have 6 protons.
Carbon-12 has 12 neutrons; Carbon-14 has 14 neutrons.

","correct":false,"explanation":"Mass numbers count protons and neutrons together, so they cannot be used directly as neutron counts. Carbon-12 and carbon-14 contain 6 and 8 neutrons respectively."},{"text":"

Both have 6 protons.
Carbon-12 has 8 neutrons; Carbon-14 has 6 neutrons.

","correct":false,"explanation":"The neutron counts have been reversed. Carbon-14 has the larger mass number and therefore has 8 neutrons, while carbon-12 has 6 neutrons."}]}]}],"examCountdown":{"examDate":"2027-05-19","paperLabel":"Paper 1"},"heading":"Atomic structure","title":"Atomic structure Flashcards","topbar":{"backHref":"/igcse/chemistry/edexcel/flashcards"},"topicSidebar":"$L36"}]}],"topicId":"ba7a88d8-8f52-5c56-8c3b-459dfc6f9a43","walled":"$L37"}],"$L38","$L39"]