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22:[["$","$L31",null,{"feature":"flashcards"}],"$L32",["$","$L33",null,{"href":"/gcse/chemistry/aqa/relative-formula-mass/flashcards","label":"3.1.2 Relative formula mass","subjectCode":"gcse_chemistry__aqa","surface":"flashcards"}],["$","$L34",null,{"runner":["$","div",null,{"className":"min-h-0 flex-1 overflow-hidden bg-background","children":["$","$L35",null,{"decks":[{"id":"c822331c-0901-4abb-938a-7351b5d23f85","title":"3.1.2 Relative formula mass Flashcards","topicId":"4d89bc46-264a-5433-9123-ed00f97d4d79","topicSlug":"relative-formula-mass","cards":[{"id":"df659a1b-86da-4d60-8564-8f5a4bae0ee5","cardType":"basic","points":1,"front":"What does relative atomic mass,

$A_r$

, compare an atom with?","back":"One twelfth of the mass of a carbon-12 atom.","mcqOptions":[{"text":"One twelfth of the mass of a carbon-12 atom.","correct":true,"explanation":"Relative atomic mass compares an atom’s mass with one twelfth of the mass of a carbon-12 atom, which is the standard reference used for atomic masses."},{"text":"The mass of one carbon-12 atom.","correct":false,"explanation":"The carbon-12 atom is divided into twelve equal parts for the comparison; using the whole atom would make the relative atomic mass twelve times too small."},{"text":"One sixth of the mass of an oxygen-16 atom.","correct":false,"explanation":"Relative atomic mass uses carbon-12 as the reference, not oxygen-16, and the reference is one twelfth of a carbon-12 atom’s mass."},{"text":"One sixteenth of the mass of a carbon-12 atom.","correct":false,"explanation":"The reference mass is one twelfth of carbon-12, not one sixteenth. The denominator twelve comes from defining carbon-12 as having a relative atomic mass of exactly 12."}]},{"id":"bec78add-cff6-4c99-b40e-7422ad2ae296","cardType":"basic","points":1,"front":"Which number beside an element symbol gives its

$A_r$

on the periodic table?","back":"The larger number.","mcqOptions":[{"text":"The larger number.","correct":true,"explanation":"The larger number beside an element symbol is usually its relative atomic mass, while the smaller whole number is the atomic number."},{"text":"The smaller number.","correct":false,"explanation":"The smaller number is the atomic number, showing the number of protons. The relative atomic mass is given by the larger number beside the element symbol."},{"text":"The group number.","correct":false,"explanation":"The group number identifies an element’s column and helps indicate its chemical properties. Its relative atomic mass is shown separately as the larger number."},{"text":"The period number.","correct":false,"explanation":"The period number identifies the row of the periodic table and relates to occupied electron shells. The larger number beside the symbol gives the relative atomic mass."}]},{"id":"6a6eb05c-de1e-4f39-9471-c234b650e2b3","cardType":"basic","points":2,"front":"Why does relative atomic mass have no units?","back":"It is a ratio comparing two masses.","mcqOptions":[{"text":"It is a ratio comparing two masses.","correct":true,"explanation":"A ratio compares two quantities of the same type, so their units cancel. Relative atomic mass therefore has no units, even though it compares masses."},{"text":"It is a mass measured in grams.","correct":false,"explanation":"Relative atomic mass is a comparison rather than an absolute mass in grams. It is a ratio of two masses, so the units cancel out."},{"text":"It is a number of atoms measured in moles.","correct":false,"explanation":"Moles measure the amount of substance, not relative atomic mass. Relative atomic mass is a unitless ratio comparing an atom’s mass with a carbon-12 standard."},{"text":"It is a force measured in newtons.","correct":false,"explanation":"Newtons measure force, which is unrelated to relative atomic mass. Relative atomic mass compares two masses as a ratio, leaving no units."}]},{"id":"e5dc38b2-9acf-41b7-a12b-6d9565af6cde","cardType":"basic","points":1,"front":"What must be added to calculate the relative formula mass,

$M_r$

, of a compound?","back":"The $$A_r$$ values of every atom shown in its formula.","mcqOptions":[{"text":"The $$A_r$$ values of every atom shown in its formula.","correct":true,"explanation":"Relative formula mass is found by considering every atom shown in the formula and adding the appropriate relative atomic mass for each one."},{"text":"The $$A_r$$ values of only the first atom shown in its formula.","correct":false,"explanation":"Ignoring the other atoms leaves out part of the compound’s mass. Every atom represented in the formula must contribute its relative atomic mass."},{"text":"The atomic numbers of every atom shown in its formula.","correct":false,"explanation":"Atomic numbers count protons and are not used to calculate relative formula mass. The calculation requires the relative atomic mass values of all atoms shown."},{"text":"The $$A_r$$ value of the whole compound shown in its formula.","correct":false,"explanation":"A compound does not have one atomic mass value to use directly. Its relative formula mass is calculated from the

$A_r$

values of every atom in the formula."}]},{"id":"bfed9a2e-7212-4ddf-90b2-f1a2afca1434","cardType":"basic","points":2,"front":"How do you calculate the

$M_r$

of a compound from its formula?","back":"

Multiply each $$A_r$$ by its number of atoms.
Add all the totals.

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

Multiply each $$A_r$$ by its number of atoms.
Add all the totals.

","correct":true,"explanation":"Each element’s relative atomic mass must first be multiplied by the number of those atoms. Adding these contributions gives the compound’s relative formula mass."},{"text":"

Add each $$A_r$$ to its number of atoms.
Multiply all the totals.

","correct":false,"explanation":"Adding an atomic mass to its atom count mixes unlike quantities, and multiplying the totals is not the required method. Multiply each

$A_r$

by its atom count, then add."},{"text":"

Multiply each $$A_r$$ by its number of atoms.
Multiply all the totals.

","correct":false,"explanation":"The individual contributions are multiplied by atom count, but they must then be added together. Multiplying the contributions produces an incorrect relative formula mass."},{"text":"

Divide each $$A_r$$ by its number of atoms.
Add all the totals.

","correct":false,"explanation":"A subscript tells you how many atoms contribute, so it requires multiplication, not division. After multiplying each $$A_r$$ by its count, add all contributions."}]},{"id":"7df6ba3b-0ac2-4da2-b0f9-84faca6915bd","cardType":"basic","points":1,"front":"Calculate the $$M_r$$ of water, $$\\text{H}_2\\text{O}$$ , using $$A_r(\\text{H})=1$$ and $$A_r(\\text{O})=16$$ .","back":"18: $$(2 \\times 1) + 16 = 18$$ .","mcqOptions":[{"text":"18: $$(2 \\times 1) + 16 = 18$$ .","correct":true,"explanation":"Water contains two hydrogen atoms and one oxygen atom, so its relative formula mass is $(2 \\times 1) + 16 = 18$."},{"text":"17: $$(1 \\times 1) + 16 = 17$$ .","correct":false,"explanation":"This counts only one hydrogen atom and misses the subscript 2 in $$\\text{H}_2\\text{O}$$ . Both hydrogen atoms contribute, giving $(2 \\times 1) + 16 = 18$."},{"text":"32: $$(2 \\times 1) + (2 \\times 16) = 34$$ .","correct":false,"explanation":"The oxygen in water has no subscript, so there is only one oxygen atom. Including two oxygen atoms is the error; the correct calculation is $(2 \\times 1) + 16 = 18$."},{"text":"19: $$(2 \\times 1) + 17 = 19$$ .","correct":false,"explanation":"This uses an incorrect relative atomic mass for oxygen. Using the stated value of 16 and two hydrogen atoms gives $(2 \\times 1) + 16 = 18$."}]},{"id":"440bc793-3177-44d3-8810-0ad5c2c23a09","cardType":"basic","points":1,"front":"Calculate the $$M_r$$ of calcium carbonate, $$\\text{CaCO}_3$$ .","back":"100: $$40 + 12 + (3 \\times 16) = 100$$ .","mcqOptions":[{"text":"100: $$40 + 12 + (3 \\times 16) = 100$$ .","correct":true,"explanation":"Calcium carbonate contains one calcium, one carbon and three oxygen atoms. Therefore, its relative formula mass is $40 + 12 + (3 \\times 16) = 100$."},{"text":"84: $$40 + 12 + (2 \\times 16) = 84$$ .","correct":false,"explanation":"This uses two oxygen atoms instead of the three shown by the subscript in $$\\text{CaCO}_3$$ . The correct calculation is $40 + 12 + (3 \\times 16) = 100$."},{"text":"148: $$40 + 12 + (6 \\times 16) = 148$$ .","correct":false,"explanation":"The oxygen subscript 3 has been doubled, as though the whole formula were doubled. There are three oxygen atoms, so the correct relative formula mass is 100."},{"text":"68: $$40 + 12 + 16 = 68$$ .","correct":false,"explanation":"This ignores the oxygen subscript and counts only one oxygen atom. Three oxygen atoms contribute $3 \\times 16$, making the correct total 100."}]},{"id":"938eca14-01f7-4497-82a4-1d2747cc741d","cardType":"basic","points":2,"front":"What does a subscript outside brackets do in a chemical formula?","back":"It multiplies every atom inside the brackets.","mcqOptions":[{"text":"It multiplies every atom inside the brackets.","correct":true,"explanation":"A subscript outside brackets applies to the entire bracketed group, so it multiplies the number of every atom inside those brackets."},{"text":"It multiplies only the last atom inside the brackets.","correct":false,"explanation":"A subscript immediately after brackets applies to the whole group, not just the final atom. Every atom inside the brackets must be multiplied by that number."},{"text":"It multiplies every atom outside the brackets.","correct":false,"explanation":"The subscript belongs to the bracketed group and affects the atoms inside it. Atoms outside the brackets are not multiplied by that subscript."},{"text":"It adds the same number of atoms outside the brackets.","correct":false,"explanation":"A subscript represents multiplication of the bracketed group, not addition of atoms elsewhere in the formula. Each atom inside the brackets occurs that many times."}]},{"id":"1b1ac777-4181-4d1b-b674-0769fafcfcae","cardType":"basic","points":1,"front":"In $$\\text{Ca(OH)}_2$$ , which atoms are multiplied by the subscript 2?","back":"Both the oxygen and hydrogen atoms inside the brackets.","mcqOptions":[{"text":"Both the oxygen and hydrogen atoms inside the brackets.","correct":true,"explanation":"The subscript 2 applies to every atom inside the brackets, so there are two oxygen atoms and two hydrogen atoms, while the calcium atom remains unmultiplied."},{"text":"Both the calcium and oxygen atoms inside the brackets.","correct":false,"explanation":"The brackets contain oxygen and hydrogen, not calcium. The subscript 2 multiplies both atoms inside the brackets, giving two oxygen atoms and two hydrogen atoms."},{"text":"Only the hydrogen atoms inside the brackets.","correct":false,"explanation":"A subscript outside brackets applies to every atom within them, not just the final element. Therefore, both oxygen and hydrogen are multiplied by 2."},{"text":"Only the calcium atoms outside the brackets.","correct":false,"explanation":"Calcium is outside the brackets, so the subscript 2 does not multiply it. The subscript applies to the oxygen and hydrogen atoms contained inside the brackets."}]},{"id":"0edcc4c2-5d4a-405a-a72f-a74771603057","cardType":"basic","points":1,"front":"Calculate the $$M_r$$ of calcium hydroxide, $$\\text{Ca(OH)}_2$$ .","back":"74: $$40 + 2 \\times (16 + 1) = 74$$ .","mcqOptions":[{"text":"74: $$40 + 2 \\times (16 + 1) = 74$$ .","correct":true,"explanation":"Calcium hydroxide contains one calcium atom, two oxygen atoms and two hydrogen atoms. Adding their relative atomic masses gives $40 + 2 \\times (16 + 1) = 74$."},{"text":"57: $$40 + 16 + 1 = 57$$ .","correct":false,"explanation":"This calculation counts only one oxygen and one hydrogen, ignoring the subscript 2 outside the brackets. Both oxygen and hydrogen must be counted twice, giving an $M_r$ of 74."},{"text":"72: $$40 + 2 \\times (16 + 2) = 76$$ .","correct":false,"explanation":"The hydrogen atomic mass is 1, not 2; 2 is the number of hydrogen atoms. Using 1 gives $40 + 2 \\times (16 + 1) = 74$."},{"text":"56: $$40 + 16 = 56$$ .","correct":false,"explanation":"This omits the hydrogen atoms and also fails to apply the bracket multiplier. Calcium hydroxide contains two oxygen and two hydrogen atoms, producing an $M_r$ of 74."}]},{"id":"18f05c83-6ba5-4235-b450-b83f394d8a8b","cardType":"basic","points":2,"front":"What does a chemical formula show about a compound?","back":"It shows the elements present and the number of atoms of each.","mcqOptions":[{"text":"It shows the elements present and the number of atoms of each.","correct":true,"explanation":"The symbols identify which elements are present, while subscripts show the number of atoms of each element in one formula unit or molecule."},{"text":"It shows the elements present and the mass of each atom.","correct":false,"explanation":"Chemical formulas use symbols and subscripts to show elements and atom numbers, not the mass of each atom. Relative atomic masses are found from a periodic table."},{"text":"It shows the number of molecules and the charge of each element.","correct":false,"explanation":"A formula does not normally give the number of molecules present, and its subscripts show atom numbers rather than each element’s charge."},{"text":"It shows the melting point and the number of atoms of each.","correct":false,"explanation":"Subscripts can show the number of atoms, but a chemical formula does not show melting point. Physical properties must be obtained from experimental data or reference information."}]},{"id":"d2e93768-7b2d-4b6d-9cf8-9c65df59f92b","cardType":"basic","points":2,"front":"In a balanced equation, how do the total relative formula masses compare on both sides?","back":"The total reactant $$M_r$$ equals the total product $$M_r$$ .","mcqOptions":[{"text":"The total reactant $$M_r$$ equals the total product $$M_r$$ .","correct":true,"explanation":"A balanced equation has the same number of each type of atom on both sides. Consequently, the total relative formula mass of the reactants equals that of the products."},{"text":"The total reactant $$M_r$$ is greater than the total product $$M_r$$ .","correct":false,"explanation":"A reaction does not lose mass when atoms are rearranged. In a balanced equation, the total relative formula mass of the reactants equals the total product relative formula mass."},{"text":"The total reactant $$M_r$$ is less than the total product $$M_r$$ .","correct":false,"explanation":"Products cannot gain mass from nowhere in a balanced chemical reaction. Conserving every atom means the total reactant relative formula mass equals the total product relative formula mass."},{"text":"The total reactant $$M_r$$ is unrelated to the total product $$M_r$$ .","correct":false,"explanation":"The two totals are directly linked by conservation of atoms and mass. A correctly balanced equation gives equal total relative formula masses on both sides."}]},{"id":"6668ff43-b06d-497b-943e-339347d401bb","cardType":"basic","points":1,"front":"For $$2\\text{Mg} + \\text{O}_2 \\rightarrow 2\\text{MgO}$$ , what is the total relative formula mass of the reactants?","back":"80: $$(2 \\times 24) + 32 = 80$$ .","mcqOptions":[{"text":"80: $$(2 \\times 24) + 32 = 80$$ .","correct":true,"explanation":"The reactants contain two magnesium atoms and one oxygen molecule. Their total relative formula mass is $(2 \\times 24) + 32 = 80$."},{"text":"112: $$2 \\times (24 + 32) = 112$$ .","correct":false,"explanation":"This incorrectly treats oxygen as if two oxygen formula units were paired with each magnesium atom. The equation has two magnesium atoms but only one oxygen molecule, giving 80."},{"text":"64: $$(2 \\times 24) + 16 = 64$$ .","correct":false,"explanation":"The oxygen molecule is $\\text{O}_2$, so its relative formula mass is $2 \\times 16 = 32$, not 16. Adding it to two magnesium atoms gives 80."},{"text":"56: $$24 + 32 = 56$$ .","correct":false,"explanation":"This counts only one magnesium atom and omits the coefficient 2. The equation contains two magnesium atoms, so the reactant total is $(2 \\times 24) + 32 = 80$."}]},{"id":"e9c9d509-796c-4a23-8c9a-a47a314dd418","cardType":"basic","points":1,"front":"For $$2\\text{Mg} + \\text{O}_2 \\rightarrow 2\\text{MgO}$$ , what is the total relative formula mass of the products?","back":"80: $$2 \\times 40 = 80$$ .","mcqOptions":[{"text":"80: $$2 \\times 40 = 80$$ .","correct":true,"explanation":"Each magnesium oxide unit has a relative formula mass of $24 + 16 = 40$. The coefficient 2 means there are two units, so the product total is $2 \\times 40 = 80$."},{"text":"40: $$24 + 16 = 40$$ .","correct":false,"explanation":"This calculates the mass of one magnesium oxide unit but ignores the coefficient 2. The equation produces two units, so the total product relative formula mass is 80."},{"text":"48: $$2 \\times 24 = 48$$ .","correct":false,"explanation":"This includes the coefficient but counts only magnesium, omitting oxygen. Each magnesium oxide unit has mass $24 + 16 = 40$, making two units total 80."},{"text":"112: $$2 \\times (24 + 32) = 112$$ .","correct":false,"explanation":"This incorrectly uses oxygen’s molecular mass, 32, inside magnesium oxide. The formula contains one oxygen atom of mass 16 per unit, so two MgO units total 80."}]},{"id":"622410ac-b90a-49c5-91f5-24e9f3dce5e6","cardType":"basic","points":1,"front":"What does matching total formula masses on both sides of a balanced equation show?","back":"Mass is conserved.","mcqOptions":[{"text":"Mass is conserved.","correct":true,"explanation":"Equal total formula masses show that the atoms have only been rearranged, not created or destroyed. Therefore, the total mass is conserved during the reaction."},{"text":"Mass is created.","correct":false,"explanation":"A reaction cannot create mass from nothing. Matching formula masses show that the original atoms are rearranged and the total mass is conserved."},{"text":"Mass is destroyed.","correct":false,"explanation":"Mass is not lost when a chemical reaction occurs in a closed system. Equal totals on both sides demonstrate conservation of mass rather than destruction."},{"text":"Energy is conserved.","correct":false,"explanation":"Matching formula masses directly demonstrate conservation of mass, not energy. Energy changes may occur during reactions, but they are not what these mass calculations establish."}]},{"id":"8941947d-d787-4812-963d-dff7eddc36c7","cardType":"cloze","points":null,"front":"Relative atomic mass, $$A_r$$ , is a weighted mean mass compared with [ ].","back":"Relative atomic mass, $$A_r$$ , is a weighted mean mass compared with one twelfth of a carbon-12 atom.","mcqOptions":[{"text":"one twelfth of a carbon-12 atom","correct":true,"explanation":"Relative atomic mass compares an atom’s weighted mean mass with one twelfth of the mass of a carbon-12 atom, the standard reference used for atomic masses."},{"text":"one carbon-12 atom","correct":false,"explanation":"A carbon-12 atom provides the reference isotope, but relative atomic mass uses one twelfth of its mass so that the carbon-12 atom has a relative mass of 12."},{"text":"one twelfth of an oxygen-16 atom","correct":false,"explanation":"Oxygen-16 is not the standard reference for relative atomic mass. The comparison is made with one twelfth of a carbon-12 atom."},{"text":"the average mass of a hydrogen atom","correct":false,"explanation":"Hydrogen is an element whose relative atomic mass can be measured, not the reference standard itself. Relative atomic mass is compared with one twelfth of carbon-12."}]},{"id":"3fa5c150-eac6-49a6-a178-214469017ea1","cardType":"cloze","points":null,"front":"Relative formula mass, $$M_r$$ , is the sum of the relative atomic masses of all the [ ].","back":"Relative formula mass, $$M_r$$ , is the sum of the relative atomic masses of all the atoms shown in the formula.","mcqOptions":[{"text":"atoms shown in the formula","correct":true,"explanation":"Relative formula mass is found by adding the relative atomic masses of every atom represented in the chemical formula, including atoms indicated by subscripts."},{"text":"elements shown in the formula","correct":false,"explanation":"The calculation counts individual atoms, not just different elements. For example, the subscript in CO₂ means two oxygen atoms must contribute to the relative formula mass."},{"text":"molecules shown in the formula","correct":false,"explanation":"A formula represents the atoms present and their numbers, rather than counting molecules. Subscripts show how many atoms of each element contribute to the total."},{"text":"bonds shown in the formula","correct":false,"explanation":"Chemical bonds do not contribute separate values to relative formula mass. Add the relative atomic masses of all the atoms shown, using subscripts to count repeated atoms."}]},{"id":"51a3da85-c2aa-49bc-8bfa-e5d61b3c5e73","cardType":"cloze","points":null,"front":"Neither $$A_r$$ nor $$M_r$$ has [ ] because each is a ratio.","back":"Neither $$A_r$$ nor $$M_r$$ has units because each is a ratio.","mcqOptions":[{"text":"units","correct":true,"explanation":"Relative atomic mass and relative formula mass are ratios comparing masses with a standard reference, so the units cancel and neither quantity has units."},{"text":"dimensions","correct":false,"explanation":"Although dimensions describe physical quantities, this is not the missing term. The correct statement is that Aᵣ and Mᵣ have no units because they are ratios."},{"text":"symbols","correct":false,"explanation":"Chemical symbols identify elements and are not something that Aᵣ or Mᵣ possesses. The quantities have no units because each is a ratio of masses."},{"text":"values","correct":false,"explanation":"Aᵣ and Mᵣ do have numerical values, even though they lack units. The missing word is units, which cancel when the mass ratio is calculated."}]},{"id":"74e6bd51-99cc-4424-9522-d3e59494c27f","cardType":"cloze","points":null,"front":"For $$\\text{Ca(OH)}_2$$ , the subscript 2 multiplies [ ] inside the brackets.","back":"For $$\\text{Ca(OH)}_2$$ , the subscript 2 multiplies both O and H inside the brackets.","mcqOptions":[{"text":"both O and H","correct":true,"explanation":"The subscript 2 applies to everything inside the brackets, so Ca(OH)₂ contains two oxygen atoms and two hydrogen atoms."},{"text":"only O","correct":false,"explanation":"The subscript outside the brackets multiplies the whole hydroxide group, not just the first element. Ca(OH)₂ therefore contains both two O atoms and two H atoms."},{"text":"only H","correct":false,"explanation":"Although H is inside the bracket, the subscript applies to the entire bracketed group. Both O and H are multiplied by 2 in Ca(OH)₂."},{"text":"Ca and O","correct":false,"explanation":"The subscript 2 is written after the brackets, so it does not multiply Ca outside them. It multiplies both elements inside the brackets: O and H."}]},{"id":"57609bc4-6e3a-4d0c-a390-b5ed635254ba","cardType":"cloze","points":null,"front":"For $$\\text{CO}_2$$ , using $$A_r(\\text{C})=12$$ and $$A_r(\\text{O})=16$$ , $$M_r = 12 + (2 \\times 16) = $$ [ ].","back":"For $$\\text{CO}_2$$ , using $$A_r(\\text{C})=12$$ and $$A_r(\\text{O})=16$$ , $$M_r = 12 + (2 \\times 16) = $$ 44.","mcqOptions":[{"text":"44","correct":true,"explanation":"Carbon contributes 12 and the two oxygen atoms contribute 2 × 16 = 32. Adding these gives Mᵣ = 12 + 32 = 44."},{"text":"28","correct":false,"explanation":"This treats CO₂ as though it contained one oxygen atom, calculating 12 + 16. The subscript 2 requires two oxygen contributions, giving the correct Mᵣ of 44."},{"text":"32","correct":false,"explanation":"This includes the mass of two oxygen atoms but omits carbon, calculating 2 × 16. Including carbon gives 12 + 32, so the correct Mᵣ is 44."},{"text":"56","correct":false,"explanation":"This commonly results from multiplying the carbon value as well as oxygen, calculating 2 × (12 + 16). Only the oxygen is doubled, so Mᵣ is 44."}]}]}],"examCountdown":{"examDate":"2027-05-17","paperLabel":"Paper 1"},"heading":"3.1.2 Relative formula mass","title":"3.1.2 Relative formula mass Flashcards","topbar":{"backHref":"/gcse/chemistry/aqa/flashcards"},"topicSidebar":"$L36"}]}],"topicId":"4d89bc46-264a-5433-9123-ed00f97d4d79","walled":"$L37"}],"$L38","$L39"]