Ions
An iodine atom forms an _________________________ ion
iodide I⁻
Minus by minus is a
+
The charge on metal ions, given that the atoms will always have lost valence shell electrons
+
Plus by a minus is a
-
The charge on non-metal ions, given that the atoms will always have gained valence shell electrons
-
The metals find in Group 1 have one valence electron. They all form ions with a ____________ charge
1+
The non-metal atoms in Group 7 require one electron to fill their valance shell's. They all form ions with a __________ charge.
1-
The metals find in Group 2 have one valence electron. They all form ions with a ____________ charge
2+
The non-metal atoms in Group 6 require two electrons to fill their valance shell's. They all form ions with a __________ charge.
2-
The electronic configuration of an aluminium atom is 2.8.3. What is the electronic configuration of an aluminium ion and what is its symbol?
2.8 Al³⁺
The electronic configuration of an fluorine atom is 2.7. What is the electronic configuration of a fluoride ion and what is its symbol?
2.8 F⁻
The electronic configuration of a magnesium atom is 2.8.2. What is the electronic configuration of a magnesium ion and what is its symbol?
2.8 Mg²⁺
The electronic configuration of a sodium atom is 2.8.1. What is the electronic configuration of a sodium ion and what is its symbol?
2.8 Na⁺
The electronic configuration of a nitrogen atom is 2.5. What is the electronic configuration of a nitride ion and what is its symbol?
2.8 N³⁻
The electronic configuration of an oxygen atom is 2.6. What is the electronic configuration of an oxide ion and what is its symbol?
2.8 O²⁻
The electronic configuration of a calcium atom is 2.8.8.2. What is the electronic configuration of a calcium ion and what is its symbol?
2.8.8 Ca²⁺
The electronic configuration of an chlorine atom is 2.8.7. What is the electronic configuration of a chloride ion and what is its symbol?
2.8.8 Cl⁻
The electronic configuration of a potassium atom is 2.8.8.1. What is the electronic configuration of a potassium ion and what is its symbol?
2.8.8 K⁺
The electronic configuration of a sulfur atom is 2.8.6. What is the electronic configuration of an sulfide ion and what is its symbol?
2.8.8 S²⁻
Aluminium is a metal finding Group 3. It forms an ion with _______ charge
3+
Nitrogen and phosphorus are non-metal atoms found in group 5. They both form ions with a ___________ charge
3-
What is an ion?
An atom that has gained or lost electrons. Unlike an atom, an ion is charged!
Why do some atoms form ion?
Atoms with an incomplete outer shell are unstable. Metal atoms, that typically have 1, 2 or 3 electrons in their outermost shell, lose all of their outer electrons. They empty out their outermost shell, forming positive ions. Non-metal atoms, that typically need 1, 2 or 3 electrons to fill their outermost shell, gain electrons and form negative ions Atoms with 4 valence electrons (C and Si) find it difficult to lose and to gain so many electrons. They rarely form ions as a result, but instead share electrons with other atoms.
Hydrogen is a non-metal atom, but it forms a positive ion. Does it lose or gain electrons?
Its atoms lose one electron to empty out the shell. Removing one electron results in the formation of an ion with a 1+ charge. Remember: a minus by a minus is a plus!
Why are negative ions larger than the atoms from which they formed?
The size of an atom or ion is controlled by how strongly the electrons are attracted by the positive protons in the nucleus. In forming a negative ion, the atom will have gained electrons. The attraction for each electron will then be weaker (as there are more electrons) and the negative ion will be smaller.
Why are positive ions smaller than the atoms from which they formed?
The size of an atom or ion is controlled by how strongly the electrons are attracted by the positive protons in the nucleus. In forming a positive ion, the atom will have lost electrons. The attraction for each remaining electron will then be stronger and the positive ion will be smaller.
The atoms of Group O (noble gases) do not form ions. Why?
They are already stable, as they have full valance shell. They do not need to gain or lose electrons.
The following are isoelectronic: Oxide ion, Fluoride ion, Neon ATOM, Sodium ion and Magnesium ion. What does 'isoelectronic' mean?
To have the same number of electrons. All 5 of these have 10 electrons. Neon ATOMS have a stable electronic configuration (2.8). The 4 ions have the same stable electronic configuration - resulting from their atoms gaining or losing electrons.
A bromine atom forms a _________________________ ion
bromide Br⁻
When drawing atoms and ions, always enclose ions in brackets (parenthesis) with the _____________ displayed as a superscript outside the brackets to the top right
charge The image shows how to draw a fluorine atom and then a fluoride ion.
A chlorine atom forms a _________________________ ion
chloride Cl⁻
Attractions between positive and negative ions are called
electrostatic attractions (ionic bonds)
A fluorine atom forms a _________________________ ion
fluoride F⁻
The elements in Group 7 are named the halogens. Their ions are named the
halide ions
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A nitrogen atom forms an ___________ ion
nitride N³⁻
An oxygen atom forms an ______________ Ion
oxide O²⁻
A phosphorus atom forms an _____________ ion
phosphide P³⁻
A sulfur atom forms an ______________ ion
sulfide S²⁻
