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

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

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 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 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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