2. properties of compounds are the same/different from the properties of the elements that make up the compound before they form a bond.
3. define the following terms:
a. chemical formula
b. subscript
c. chemical bond
4. atoms become more stable when they _______, _______, or _______ their valence electrons.
5. when an atom loses electrons, it becomes a positive/negative ion.
6. when an atom gains electrons, it becomes a positive/negative ion.
7. a positive ion has more _______ than _______.
8. a negative ion has more _______ than _______.
9. which group numbers of the periodic table lose electrons and form cations?
10. which group numbers of the periodic table gain electrons and form anions?

Question

2. properties of compounds are the same/different from the properties of the elements that make up the compound before they form a bond.
3. define the following terms:
   a. chemical formula
   b. subscript
   c. chemical bond
4. atoms become more stable when they _______, _______, or _______ their valence electrons.
5. when an atom loses electrons, it becomes a positive/negative ion.
6. when an atom gains electrons, it becomes a positive/negative ion.
7. a positive ion has more _______ than _______.
8. a negative ion has more _______ than _______.
9. which group numbers of the periodic table lose electrons and form cations?
10. which group numbers of the periodic table gain electrons and form anions?

Accepted Answer

### Question 2
# Brief Explanations:
Compounds have distinct properties from their constituent elements. For example, sodium (a reactive metal) and chlorine (a toxic gas) form sodium chloride (table salt, safe and stable), so properties are different.
# Answer:
different

### Question 3a
# Brief Explanations:
A chemical formula uses symbols and subscripts to represent the composition of a compound or molecule, e.g., $H_2O$ for water (2 H, 1 O).
# Answer:
A chemical formula is a notation using chemical symbols and numerical subscripts to represent the composition of a compound (or molecule), indicating the types and relative numbers of atoms of each element present.

### Question 3b
# Brief Explanations:
In a chemical formula, a subscript is a small number below and to the right of an element symbol, showing the number of atoms of that element in a molecule or formula unit, e.g., the 2 in $H_2O$ means 2 hydrogen atoms.
# Answer:
A subscript is a small number written below and to the right of an element’s symbol in a chemical formula, indicating the number of atoms of that element in a molecule (or formula unit of an ionic compound).

### Question 3c
# Brief Explanations:
A chemical bond is the force that holds atoms together in a compound, formed by electron sharing (covalent) or transfer (ionic), stabilizing atoms by achieving a full valence shell.
# Answer:
A chemical bond is the attractive force that holds two or more atoms together in a molecule (or formula unit of an ionic compound), resulting from interactions between the atoms’ valence electrons (e.g., through electron transfer in ionic bonds or electron sharing in covalent bonds).

### Question 4
# Brief Explanations:
Atoms stabilize by achieving a full valence shell (like noble gases). They can lose, gain, or share valence electrons: metals lose, nonmetals gain, and some share (covalent bonding).
# Answer:
lose, gain, share

### Question 5
# Brief Explanations:
Losing electrons means the atom has more protons (positive charge) than electrons (negative charge), so it becomes a positive ion (cation), e.g., Na loses an electron to become $Na^+$.
# Answer:
positive

### Question 6
# Brief Explanations:
Gaining electrons adds negative charge, so the atom has more electrons than protons, forming a negative ion (anion), e.g., Cl gains an electron to become $Cl^-$.
# Answer:
negative

### Question 7
# Brief Explanations:
A positive ion (cation) forms when an atom loses electrons. Protons are positive, electrons negative. If electrons are lost, protons (positive) outnumber electrons (negative), so more protons than electrons.
# Answer:
protons, electrons

### Question 8
# Brief Explanations:
A negative ion (anion) forms when an atom gains electrons. Gaining electrons means the number of electrons (negative) exceeds protons (positive), so more electrons than protons.
# Answer:
electrons, protons

### Question 9
# Brief Explanations:
Groups 1, 2, and 13 (or 3A) in the periodic table are metals (or metal - like) that tend to lose electrons to form cations. Group 1 (alkali metals) lose 1 electron, Group 2 (alkaline earths) lose 2, and Group 13 (e.g., Al) lose 3, forming $Na^+$, $Mg^{2+}$, $Al^{3+}$ etc.
# Answer:
Groups 1, 2, and 13 (or 3A) of the periodic table (alkali metals, alkaline earth metals, and some from Group 13) lose electrons to form cations.

### Question 10
# Brief Explanations:
Groups 15, 16, 17 (or 5A, 6A, 7A) are nonmetals that gain electrons to form anions. Group 17 (halogens) gain 1 electron ($Cl^-$), Group 16 gain 2 ($O^{2 -}$), Group 15 gain 3 ($N^{3 -}$) to achieve a full valence shell.
# Answer:
Groups 15, 16, and 17 (or 5A, 6A, 7A) of the periodic table (nonmetals in these groups) gain electrons to form anions.

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