teacher demo: synthesis
1. magnesium
__mg + __o₂ → _______
2. salt
__na + __cl₂ → _______
teacher demo: decomposition
1. elephant toothpaste
__h₂o₂ →
2. gummy bear (please remind me that i need someone to melt this while i do the other demo:))
__kclo₃ →
predict the product(s) for the following synthesis reactions and balance the equation.
1. __ca + __o₂ →
2. __zn + __n₂ →
3. __al + __cl₂ →
predict the product(s) for the following decomposition and balance the equation
1. __mgo →
2. __kcl →
3. __nacl →
write the balanced chemical equation
1. magnesium reacts with sulfur to form magnesium sulfide.
2. sulfur reacts with oxygen gas to form sulfur trioxide.
3. magnesium carbonate decomposes to produce magnesium oxide and carbon dioxide.

Question

Accepted Answer

### Teacher Demo: Synthesis
#### 1. Magnesium
# Explanation:
## Step1: Identify reaction type (synthesis)
Magnesium (Mg) reacts with oxygen ($O_2$) to form magnesium oxide (MgO).
## Step2: Balance the equation
Count atoms: Mg: 1, O: 2 on left. Mg: 1, O: 1 on right (for MgO). To balance O, put 2 in front of MgO: $Mg + O_2
ightarrow 2MgO$. Now Mg: 1 vs 2. Put 2 in front of Mg: $2Mg + O_2
ightarrow 2MgO$.
# Answer:
$2$Mg + $1$O₂ → $2$MgO

#### 2. Salt
# Explanation:
## Step1: Identify reaction type (synthesis)
Sodium (Na) reacts with chlorine ($Cl_2$) to form sodium chloride (NaCl).
## Step2: Balance the equation
Count atoms: Na: 1, Cl: 2 on left. Na: 1, Cl: 1 on right (for NaCl). To balance Cl, put 2 in front of NaCl: $Na + Cl_2
ightarrow 2NaCl$. Now Na: 1 vs 2. Put 2 in front of Na: $2Na + Cl_2
ightarrow 2NaCl$.
# Answer:
$2$Na + $1$Cl₂ → $2$NaCl

### Teacher Demo: Decomposition
#### 1. Elephant toothpaste (Hydrogen Peroxide Decomposition)
# Explanation:
## Step1: Identify reaction type (decomposition)
Hydrogen peroxide ($H_2O_2$) decomposes into water ($H_2O$) and oxygen ($O_2$).
## Step2: Balance the equation
Unbalanced: $H_2O_2
ightarrow H_2O + O_2$. Count O: 2 (left) vs 3 (right: 1 in $H_2O$, 2 in $O_2$). Multiply $H_2O_2$ by 2, $H_2O$ by 2: $2H_2O_2
ightarrow 2H_2O + O_2$. Now H: 4 (left) = 4 (right), O: 4 (left) = 2 + 2 (right). Balanced.
# Answer:
$2$H₂O₂ → $2$H₂O + $1$O₂

#### 2. Gummy bear (Potassium Chlorate Decomposition)
# Explanation:
## Step1: Identify reaction type (decomposition)
Potassium chlorate ($KClO_3$) decomposes into potassium chloride (KCl) and oxygen ($O_2$).
## Step2: Balance the equation
Unbalanced: $KClO_3
ightarrow KCl + O_2$. Count O: 3 (left) vs 2 (right). Find LCM of 3 and 2 (6). Multiply $KClO_3$ by 2, $O_2$ by 3: $2KClO_3
ightarrow KCl + 3O_2$. Now K: 2, Cl: 2 on left; K: 1, Cl: 1 on right. Multiply KCl by 2: $2KClO_3
ightarrow 2KCl + 3O_2$. Balanced.
# Answer:
$2$KClO₃ → $2$KCl + $3$O₂

### Predict the product(s) and balance (Synthesis Reactions)
#### 1. Calcium + Oxygen
# Explanation:
## Step1: Predict product (synthesis)
Calcium (Ca) + Oxygen ($O_2$) → Calcium Oxide (CaO).
## Step2: Balance
Unbalanced: $Ca + O_2
ightarrow CaO$. O: 2 vs 1. Multiply CaO by 2: $Ca + O_2
ightarrow 2CaO$. Ca: 1 vs 2. Multiply Ca by 2: $2Ca + O_2
ightarrow 2CaO$.
# Answer:
$2$Ca + $1$O₂ → $2$CaO

#### 2. Zinc + Nitrogen
# Explanation:
## Step1: Predict product (synthesis)
Zinc (Zn) + Nitrogen ($N_2$) → Zinc Nitride ($Zn_3N_2$) (metal + nonmetal → ionic compound).
## Step2: Balance
Unbalanced: $Zn + N_2
ightarrow Zn_3N_2$. Zn: 1 vs 3, N: 2 vs 2. Multiply Zn by 3: $3Zn + N_2
ightarrow Zn_3N_2$.
# Answer:
$3$Zn + $1$N₂ → $1$Zn₃N₂

#### 3. Aluminum + Chlorine
# Explanation:
## Step1: Predict product (synthesis)
Aluminum (Al) + Chlorine ($Cl_2$) → Aluminum Chloride ($AlCl_3$) (metal + nonmetal → ionic compound).
## Step2: Balance
Unbalanced: $Al + Cl_2
ightarrow AlCl_3$. Cl: 2 vs 3. LCM of 2 and 3 is 6. Multiply $Cl_2$ by 3, $AlCl_3$ by 2: $Al + 3Cl_2
ightarrow 2AlCl_3$. Al: 1 vs 2. Multiply Al by 2: $2Al + 3Cl_2
ightarrow 2AlCl_3$.
# Answer:
$2$Al + $3$Cl₂ → $2$AlCl₃

### Predict the product(s) and balance (Decomposition Reactions)
#### 1. Magnesium Oxide
# Explanation:
## Step1: Predict product (decomposition)
Magnesium Oxide (MgO) decomposes into Magnesium (Mg) and Oxygen ($O_2$) (ionic compound → metal + nonmetal).
## Step2: Balance
Unbalanced: $MgO
ightarrow Mg + O_2$. O: 1 vs 2. Multiply MgO by 2: $2MgO
ightarrow Mg + O_2$. Mg: 2 vs 1. Multiply Mg by 2: $2MgO
ightarrow 2Mg + O_2$.
# Answer:
$2$MgO → $2$Mg + $1$O₂

#### 2. Potassium Chloride
# Explanation:
## Step1: Predict product (decomposition)
Potassium Chloride (KCl) is an ionic compound of Group 1 metal and halogen. It decomposes into Potassium (K) and Chlorine ($Cl_2$) (but KCl is stable; for balancing practice, assume decomposition: $KCl
ightarrow K + Cl_2$).
## Step2: Balance
Unbalanced: $KCl
ightarrow K + Cl_2$. Cl: 1 vs 2. Multiply KCl by 2: $2KCl
ightarrow K + Cl_2$. K: 2 vs 1. Multiply K by 2: $2KCl
ightarrow 2K + Cl_2$.
# Answer:
$2$KCl → $2$K + $1$Cl₂

#### 3. Sodium Chloride
# Explanation:
## Step1: Predict product (decomposition)
Sodium Chloride (NaCl) decomposes into Sodium (Na) and Chlorine ($Cl_2$) (ionic compound → metal + nonmetal).
## Step2: Balance
Unbalanced: $NaCl
ightarrow Na + Cl_2$. Cl: 1 vs 2. Multiply NaCl by 2: $2NaCl
ightarrow Na + Cl_2$. Na: 2 vs 1. Multiply Na by 2: $2NaCl
ightarrow 2Na + Cl_2$.
# Answer:
$2$NaCl → $2$Na + $1$Cl₂

### Write Balanced Chemical Equations
#### 1. Magnesium + Sulfur → Magnesium Sulfide
# Explanation:
## Step1: Identify reactants/products
Reactants: Mg, S (sulfur is $S_8$? No, for simplicity, use S as diatomic? Wait, sulfur is often $S$ (atomic) in synthesis with metals. Product: MgS.
## Step2: Balance
Unbalanced: $Mg + S
ightarrow MgS$. Atoms: Mg:1, S:1 on both sides. Wait, but sulfur is $S_8$? No, the problem says "sulfur" (assume atomic S for simplicity). So balanced as $Mg + S
ightarrow MgS$. But if S is $S_8$, adjust: $8Mg + S_8
ightarrow 8MgS$. But the problem likely uses S (atomic). So:
# Answer:
$1$Mg + $1$S → $1$MgS (or if S is $S_8$: $8$Mg + $1$S₈ → $8$MgS)

#### 2. Sulfur + Oxygen → Sulfur Trioxide
# Explanation:
## Step1: Identify reactants/products
Reactants: S, $O_2$; Product: $SO_3$.
## Step2: Balance
Unbalanced: $S + O_2
ightarrow SO_3$. Count O: 2 vs 3. LCM of 2 and 3 is 6. Multiply $O_2$ by 3, $SO_3$ by 2: $S + 3O_2
ightarrow 2SO_3$. S: 1 vs 2. Multiply S by 2: $2S + 3O_2
ightarrow 2SO_3$.
# Answer:
$2$S + $3$O₂ → $2$SO₃

#### 3. Magnesium Carbonate → Magnesium Oxide + Carbon Dioxide
# Explanation:
## Step1: Identify reactants/products
Reactant: $MgCO_3$; Products: $MgO$, $CO_2$.
## Step2: Balance
Unbalanced: $MgCO_3
ightarrow MgO + CO_2$. Count atoms: Mg:1, C:1, O:3 (left); Mg:1, C:1, O:1 + 2 = 3 (right). Already balanced.
# Answer:
$1$MgCO₃ → $1$MgO + $1$CO₂

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QUESTION IMAGE

Question

Explanation:

Teacher Demo: Synthesis

1. Magnesium

Step1: Identify reaction type (synthesis)

Step2: Balance the equation

Step1: Identify reaction type (synthesis)

Step2: Balance the equation

Step1: Identify reaction type (decomposition)

Step2: Balance the equation

Answer:

2. Salt