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

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R E L A T I V E F O R M U L A M A S S J I
P X X Y K M R O D C F U J W C A F S E A R
L N M H C C A T O M I C N U M B E R A Y O
R V Y O T C C O N C E N T R A T I O N W H
V L J W U Y H J W V S R C S W D H O U A O
I B I N N J M H U V E G O D B X X A S W D
A M O U N T O F S U B S T A N C E E B T E
L W U W Q M V T E F K G U R B E B Q P W L
Y M Q O X O T Q P E O B Q M W K J A W J W
H I D Q V M O L A R V O L U M E O H O Y F
Y J S T A N D A R D S O L U T I O N U C J
K E Q I Q P R I Y U L M D D O L B R T V I
M O L E C U L A R F O R M U L A B B F B A
Y G G E M P I R I C A L F O R M U L A K N
G S M Y O G U M A S S N U M B E R V C T G
C X G E B P V I K Q L Q I X B I P E C F O
R E L A T I V E I S O T O P I C M A S S V
G T M B T Q D T P L V E I X K B Q D S H N
X U S S P C Q D K M Q X Q D I T P T C X N
N V R C O R W Y N O M W X J E R I B V P E
A E V Y E X I O N Q M Y F Y J Y N E J U 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 mass of an atom of an isotope compared with one-twelfth of the mean mass of an atom of carbon-12. (8, 8, 4)
  • The number of particles in the nuclues. (4, 6)
  • 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 volume per mole os a gas. The units of molar volume are dm3 mol-1. At room temperature and pressure, the molar volume is approximately 24.0dm3mol-1. (5, 6)
  • The weighted mean mass of a formula unit compared with one-twelfth of the mass of an atom of carbon-12. (8, 7, 4)

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