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Particla Diagrams:
Be able to identify:
Pure element
Mixture of two elements
pure compound
Mixture of two compounds
mixture of element and a compounds
TYpes of Mixtures (Differences)
Homogeneous Mixtures
Heterogeneous Mixtures
Seperating Mixtures
Decanting
Chromatography
Pure Substances
Elements
Compounds
Physical Changes vs Chemical Changes
Physical Changes-Identity statys the same
Chemical Changes-New substance formed
States of Matter
Solid
Liquid
Gas
Phase Changes
Freezing
Boiling
Evaporation
Sublimation
Deposition
Melting
Solubility & Solutions
Solubility
Solute
Solvent
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Here is a concise study guide covering each item you listed. Use it to interpret particle diagrams, classify substances, understand mixtures and separations, and review changes of state and solubility.
1) Particle diagrams — how to identify
- Pure element
- All particles are identical single atoms (same color/shape), not bonded to different types.
- Example: all red single dots.
- Mixture of two elements
- Two kinds of single atoms present (two colors/shapes), not chemically bonded to each other.
- Example: red dots and blue dots randomly mixed.
- Pure compound
- Every particle is a molecule with the same bonded pattern (e.g., two different colored dots connected together repeatedly).
- Example: every particle is a blue–red pair.
- Mixture of two compounds
- Two distinct molecular species (two different bonded patterns) are present together.
- Example: some particles are blue–red pairs and others are green–yellow pairs.
- Mixture of element and compound
- Some single atoms (one color) present along with molecular particles (bonded groups).
- Example: red single dots + blue–yellow bonded pairs.
Tip: Look for bonding (lines or touching pairs) and uniformity. If every particle looks the same molecule → pure compound. If you see different unbonded atom types → elemental mixture, etc.
2) Types of mixtures (differences)
- Homogeneous mixture (solution)
- Composition is uniform at molecular scale; cannot see different parts.
- Example: sugar dissolved in water, air.
- Heterogeneous mixture
- Composition is not uniform; different regions/phases are visible.
- Example: sand in water, salad dressing (oil and vinegar).
3) Separating mixtures — common methods and when to use
- Decanting
- Pouring off the top liquid from a settled solid or immiscible liquid; works when phases separate by density (e.g., sand settled in water, oil on water).
- Filtration
- Separates solid particles from a liquid using a porous barrier (e.g., sand/water).
- Distillation
- Uses boiling point differences to separate liquids (e.g., ethanol/water).
- Evaporation / Crystallization
- Remove solvent to leave dissolved solids (e.g., salt from saltwater).
- Chromatography
- Separates substances based on different affinities to a stationary phase versus a mobile phase (paper, thin-layer, column). Good for separating dissolved pigments, amino acids, etc.
- The component that interacts less with the stationary phase moves farther with the mobile phase.
- Centrifugation
- Uses rapid spinning to separate components by density when gravity separation is too slow.
Choose method based on physical properties (density, solubility, particle size, boiling point, polarity).
4) Pure substances
- Elements
- Made of one type of atom; cannot be broken down chemically into simpler substances (e.g., O2 gas considered an element though diatomic).
- Compounds
- Two or more elements chemically bonded in fixed ratios; properties different from constituent elements (e.g., H2O).
5) Physical changes vs chemical changes
- Physical change
- Identity/composition stays the same; changes in form, phase, shape, or arrangement (e.g., melting, freezing, dissolving physically if no reaction).
- Often reversible.
- Chemical change (chemical reaction)
- New substance(s) formed; bonds broken and new bonds formed (e.g., rusting of iron, combustion).
- Signs: color change, gas evolution (bubbles not from boiling), formation of precipitate, temperature change (exo/endothermic), irreversible chemical composition change.
6) States of matter — particle behavior
- Solid
- Particles tightly packed, fixed shape, definite volume, vibrate in place.
- Liquid
- Particles close but can move/slide past each other, definite volume, shape of container.
- Gas
- Particles far apart, move freely, no definite shape or volume (expand to fill container).
7) Phase changes (definitions)
- Freezing: liquid → solid (energy released).
- Melting (fusion): solid → liquid (energy absorbed).
- Boiling: liquid → gas (bubbles throughout liquid; energy absorbed).
- Evaporation: liquid → gas from the surface (can occur below boiling point).
- Sublimation: solid → gas (skips liquid; e.g., dry ice).
- Deposition: gas → solid (reverse of sublimation).
8) Solubility & solutions
- Solubility
- Maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature/pressure.
- Units: g solute per 100 g solvent, mol/L, etc.
- Solute
- Substance being dissolved (smaller amount).
- Solvent
- Substance doing the dissolving (larger amount; often water = “universal solvent”).
- Saturated vs Unsaturated vs Supersaturated
- Saturated: contains maximum dissolved solute at that temperature.
- Unsaturated: more solute can dissolve.
- Supersaturated: contains more dissolved solute than normal at that temperature (unstable).
Factors affecting solubility: temperature (most solids: solubility ↑ with T; gases: solubility ↓ with T), pressure (mainly affects gases), polarity (like dissolves like: polar solvents dissolve polar solutes).
Short exam tips
- For particle diagrams: count distinct particle types and look for bonding patterns and uniformity.
- For mixtures: homogeneous = looks uniform at the particle level; heterogeneous = distinct clusters/phases.
- For separations: match method to physical property difference (density → decanting, boiling point → distillation, polarity/adsorption → chromatography).
- For changes: ask “is a new substance formed?” to distinguish chemical vs physical.
If you want, I can draw or describe specific particle diagrams and walk through classification step-by-step.
1) Particle diagrams — how to identify
- Pure element
- All particles are identical single atoms (same color/shape), not bonded to different types.
- Example: all red single dots.
- Mixture of two elements
- Two kinds of single atoms present (two colors/shapes), not chemically bonded to each other.
- Example: red dots and blue dots randomly mixed.
- Pure compound
- Every particle is a molecule with the same bonded pattern (e.g., two different colored dots connected together repeatedly).
- Example: every particle is a blue–red pair.
- Mixture of two compounds
- Two distinct molecular species (two different bonded patterns) are present together.
- Example: some particles are blue–red pairs and others are green–yellow pairs.
- Mixture of element and compound
- Some single atoms (one color) present along with molecular particles (bonded groups).
- Example: red single dots + blue–yellow bonded pairs.
Tip: Look for bonding (lines or touching pairs) and uniformity. If every particle looks the same molecule → pure compound. If you see different unbonded atom types → elemental mixture, etc.
2) Types of mixtures (differences)
- Homogeneous mixture (solution)
- Composition is uniform at molecular scale; cannot see different parts.
- Example: sugar dissolved in water, air.
- Heterogeneous mixture
- Composition is not uniform; different regions/phases are visible.
- Example: sand in water, salad dressing (oil and vinegar).
3) Separating mixtures — common methods and when to use
- Decanting
- Pouring off the top liquid from a settled solid or immiscible liquid; works when phases separate by density (e.g., sand settled in water, oil on water).
- Filtration
- Separates solid particles from a liquid using a porous barrier (e.g., sand/water).
- Distillation
- Uses boiling point differences to separate liquids (e.g., ethanol/water).
- Evaporation / Crystallization
- Remove solvent to leave dissolved solids (e.g., salt from saltwater).
- Chromatography
- Separates substances based on different affinities to a stationary phase versus a mobile phase (paper, thin-layer, column). Good for separating dissolved pigments, amino acids, etc.
- The component that interacts less with the stationary phase moves farther with the mobile phase.
- Centrifugation
- Uses rapid spinning to separate components by density when gravity separation is too slow.
Choose method based on physical properties (density, solubility, particle size, boiling point, polarity).
4) Pure substances
- Elements
- Made of one type of atom; cannot be broken down chemically into simpler substances (e.g., O2 gas considered an element though diatomic).
- Compounds
- Two or more elements chemically bonded in fixed ratios; properties different from constituent elements (e.g., H2O).
5) Physical changes vs chemical changes
- Physical change
- Identity/composition stays the same; changes in form, phase, shape, or arrangement (e.g., melting, freezing, dissolving physically if no reaction).
- Often reversible.
- Chemical change (chemical reaction)
- New substance(s) formed; bonds broken and new bonds formed (e.g., rusting of iron, combustion).
- Signs: color change, gas evolution (bubbles not from boiling), formation of precipitate, temperature change (exo/endothermic), irreversible chemical composition change.
6) States of matter — particle behavior
- Solid
- Particles tightly packed, fixed shape, definite volume, vibrate in place.
- Liquid
- Particles close but can move/slide past each other, definite volume, shape of container.
- Gas
- Particles far apart, move freely, no definite shape or volume (expand to fill container).
7) Phase changes (definitions)
- Freezing: liquid → solid (energy released).
- Melting (fusion): solid → liquid (energy absorbed).
- Boiling: liquid → gas (bubbles throughout liquid; energy absorbed).
- Evaporation: liquid → gas from the surface (can occur below boiling point).
- Sublimation: solid → gas (skips liquid; e.g., dry ice).
- Deposition: gas → solid (reverse of sublimation).
8) Solubility & solutions
- Solubility
- Maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature/pressure.
- Units: g solute per 100 g solvent, mol/L, etc.
- Solute
- Substance being dissolved (smaller amount).
- Solvent
- Substance doing the dissolving (larger amount; often water = “universal solvent”).
- Saturated vs Unsaturated vs Supersaturated
- Saturated: contains maximum dissolved solute at that temperature.
- Unsaturated: more solute can dissolve.
- Supersaturated: contains more dissolved solute than normal at that temperature (unstable).
Factors affecting solubility: temperature (most solids: solubility ↑ with T; gases: solubility ↓ with T), pressure (mainly affects gases), polarity (like dissolves like: polar solvents dissolve polar solutes).
Short exam tips
- For particle diagrams: count distinct particle types and look for bonding patterns and uniformity.
- For mixtures: homogeneous = looks uniform at the particle level; heterogeneous = distinct clusters/phases.
- For separations: match method to physical property difference (density → decanting, boiling point → distillation, polarity/adsorption → chromatography).
- For changes: ask “is a new substance formed?” to distinguish chemical vs physical.
If you want, I can draw or describe specific particle diagrams and walk through classification step-by-step.
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