Atoms and Reactions - Part 1, As, Unit 1, Module 1

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C M Q R G L X J C A J K Y W H P C O O D X
B J A M O U N T O F S U B S T A N C E I E
U R E L A T I V E A T O M I C M A S S T S
L S T A N D A R D S O L U T I O N F R F U
Q R E L A T I V E F O R M U L A M A S S I
D V H X W N N R F E S E R E A I A O K K X
T K N Q W P V Q V H W G I L T I U R O G Y
G Q G J E M C O N C E N T R A T I O N L S
P M L L A J E Y V R A U P J O Y I C M G U
W M A S W A T O M I C N U M B E R N B Q S
M G V X D P G O J Q X T Y A E R A P W C J
D S T O I C H I O M E T R Y C O X J V L H
X M E M P I R I C A L F O R M U L A J U B
A W I R O M V P E K M M K U F U R E T S A
W Q A N R P M U B F N X D W O O F T F R P
S A Q M O L E C U L A R F O R M U L A C U
J U V I D D S Q Y D B C D Q K D K P I L B
M B B Q D T L D G W T H R V Q B F L T L J
B T H E A V O G A D R O C O N S T A N T B
X B Q F G V R V I T B W L T F X G V T N L
A M I O K W P V J D X B U K S L F Q J X M

Clues

  • a solution of a known concentration. Standard solutions are normally used in titrations to determine unknown information about another substance. (8, 8)
  • The actual number of atoms of each element in a molecule. (9, 7)
  • The amount of solute, in mol, dissolved per 1 dm3 of solution. (13)
  • the molar relationship between the relative quantities of substance taking part in the reaction. (13)
  • The number of atoms per mole of the carbon-12 isotope (6.02x10^23 mol^-1). (3, 8, 8)
  • The number of protons in the nucleus of an atom. (6, 6)
  • THe quantity whose unit is the mole. Chemists use 'amount of substance' as a means of counting atoms. (6, 2, 9)
  • The simplest whole-number ratio of atoms of each element present in a compound. (9, 7)
  • The weighted mean mass of a formula unit compared with one-twelfth of the mass of an atom of carbon-12. (8, 7, 4)
  • The weighted mean mass of an atom of an element compared with one-twelfth of the mass oof an atom of carbon-12 (8, 6, 4)

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