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level: Level 1

Questions and Answers List

level questions: Level 1

Question	Answer
a stable particle with positive charge equal to the negative charge of an electron	PROTON
an elementary particle with 0 charge and mass about equal to a proton; enters into the structure of the atomic nucleus	NEUTRON
an elementary particle with negative charge	ELECTRON
an orbit followed by electrons around an a atom	ELECTRON SHELL
the outer shell of an atom	VALENCE SHELL
the electrons on the outer shell	VALENCE ELECTRON
vertical column in the periodic table	GROUP
horizontal column on a periodic table	PERIOD
the number of protons and nucleus of an atom	ATOMIC NUMBER
the total number of protons and neutrons in a neutron	MASS NUMBER
an atom with an electric charge due to the loss or gain of one of more electrons	ION
carbon ~ (2,4)	ELECTRON CONFIGURATIONS
noble gases, halogen, alkali metal, alkali earth metal, non-metal	TYPES OF ELEMENTS
alkali metals e.g. hydrogen	WHAT IS GROUP ONE KNOWN AS
alkali earth metals e.g. calcium	WHAT IS GROUP TWO KNOWN AS
non-metals e.g. iron	WHAT IS THREE ~ TWELVE KNOWN AS
halogen gases e.g. chlorine	WHAT IS GROUP 17 KNOWN AS
noble gases e.g. helium	WHAT IS GROUP 18 KNOWN AS
on the left hand side of the table, the reactivity increases as you go down the column(alkali) but if you go down the columns more on the right, the reactivity decreases (noble gases)	WHAT HAPPENS TO THE REACTIVITY OF ELEMENTS AS YOU MOVE DOWN THE GROUP?
noble gases	WHICH GROUP OF ELEMENTS HAS A FULL VALENCE ELECTRON
ions form to help make an atom more stable whether that is by losing or gaining valence electrons	WHY DO IONS FORM
formed when one atom accepts or donates one or more of its valence electrons. formed between metals and non metals e.g. NaCl, MgO, CaCo3	IONIC BONDING
formed when atoms share valence electrons. The atoms do not always share the electrons equally, so a polar covalent bond may be the result. form between non-metals and hydrogen	COVALENT BONDING
metal atoms fom close-packed, regular arrangement. The atoms 'lose' their valence electrons to become positive ions. the outerr electrons become a 'sea' of delocalised electrons surrounding a lattice of positive ions. the latticeis held together by strong electrostatic forces.	METALLIC BONDING
salt + water e.g. H2SO4 NaOH-> Na2SO4H20	ACID + BASE =
salt + carbon dioxide + water	ACID + CARBONATE =
when two elements are present the metal is named first the compound will end in 'ide' -if both are non metals and one is hydrogen, hydrogen is written first. e.g. KBr - potassium bromide CaS - calcium sulfide	WHAT IS RULE ONE ?
when two or more element combine with oxygen *the metal is named first - the compound ends with part of the name of the 2nd element combined with 'ate' or 'ite' e.g. Na2CO3 - sodium carbonate ZnSO3 - zinc sulfite	WHAT IS RULE TWO ?
when there are only 2 elements and both are non-metals hydrogen is written first, i present prefixes are joined to the name of the element to show how many atoms there are 1 - mono 4 - tetra 2 - di 5 - penta 3 - tri 6 - hexa	WHAT IS RULE 3 ?
1. carbon oxide 2. sulfur trioxide 3. hydrogen bromide 4. diphosphorus pentabromide	EXAMPLES OF PREFIXES - CO2, SO3, HBr, P2Cl5
hydrogen sulfate	WHAT IS THIS TERM - H2SO4
copper sulfate	WHAT IS THIS TERM - CuSO4
sulfur dioxide	WHAT IS THIS TERM - SO2
carbon monoxide	WHAT IS THIS TERM - CO
nitrogen trioxide	WHAT IS THIS TERM - NO3