States, boiling point,_melting_point,
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The document defines the three states of matter as solid, liquid, and gas. It explains that states of matter are defined by whether they maintain a definite shape and volume. Solids maintain a definite shape and volume, liquids have a definite volume but no defined shape, and gases do not have a definite shape or volume. The document also discusses melting point, boiling point, and solubility. Melting point is the specific temperature when a substance changes from a solid to a liquid, and boiling point is the temperature when a liquid changes to a gas. Solubility refers to the maximum amount of a substance that can dissolve in a liquid.
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Matter can exist in three states - solid, liquid, and gas. Examples of solids are ice and diamonds; examples of liquids are water and mercury. Gases include water vapor and oxygen. Characteristic properties like boiling point and melting point are used to identify substances and do not change, even if the substance changes state. Physical changes alter the substance's form through processes like melting or crushing, but do not change its chemical makeup. Chemical changes form new substances through chemical reactions.
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This document discusses the physical properties and behavior of matter. It defines the three states of matter as solids, liquids, and gases. Solids have a definite shape and volume, liquids have a definite volume but take the shape of their container, and gases fill their container uniformly with no definite shape or volume. The document also explains several gas laws including Boyle's law relating pressure and volume, Charles' law relating volume and temperature, and the combined gas law. It introduces the kinetic molecular theory as a model to explain gas behavior in terms of particle motion and interactions.
phasechanges.pptx
The document discusses the three phases of matter - solid, liquid, and gas - and phase changes between these states. A phase change is a physical change where the state of matter changes from solid to liquid to gas or vice versa. During a phase change, heat energy is either absorbed or released as molecules change their arrangement and kinetic or potential energy levels. Specific phase changes like melting, freezing, boiling, evaporation, condensation, sublimation, and deposition are explained in detail.
Lecture 2 (1)
This document discusses the classification and properties of matter. It defines matter as anything that has mass and takes up space. Matter can be classified on the macroscopic, microscopic, and sub-microscopic scales. At the sub-microscopic scale, all matter is made up of atoms. The document discusses physical and chemical properties and changes. It also introduces mixtures, compounds, elements and discusses how matter can be classified and separated.
11 particulate model (changes in state & temp curves)
The document discusses heating and cooling curves. It explains that a heating curve plots the changes in a substance's state as temperature increases over time, identifying fixed points like melting and boiling points. A cooling curve similarly plots changes as temperature decreases. The curves allow identification of a substance's state at a given temperature or time. Examples of heating and cooling curves for water and alcohol are provided.
Chapt 1 kpt of solids, liquids & gases (1)
This document describes the kinetic particle theory and the changes of state between solids, liquids, and gases. It explains that all matter is made of particles in constant motion. In solids, particles are packed closely together in a fixed pattern, in liquids they are more loosely packed but still in contact, and in gases they are far apart with little attraction. Changes between these states, like melting, boiling, condensation, and freezing occur when heating or cooling causes particles to gain or lose energy and change their motion and arrangement. The document provides detailed explanations of each state and phase change using the kinetic particle theory model.
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States, boiling point,_melting_point,
- 1. States, Boiling Point, Melting Point, and Solubility Solid Liquid Gas
- 2. Questions • What are the 3 states of matter? • Write a definition for each state?
- 3. Defining States of Matter • States of matter are NOT defined by what they are made of. – Example: solids can be elements (gold), compounds (Salt = NaCl), or mixtures (butter) Element (Au) Compound (NaCl) Mixture (Milk, Salt, etc)
- 4. Defining States of Matter • States of matter are defined by whether they hold SHAPE and VOLUME Element (Au) Compound (NaCl) Mixture (Milk, Salt, etc) ALL KEEP THE SAME SHAPE AND VOLUME = Solids
- 5. Defining States of Matter • Solids – have a definite SHAPE and VOLUME. Element (Au) Compound (NaCl) Mixture (Milk, Salt, etc) ALL KEEP THE SAME SHAPE AND VOLUME
- 6. Particle View of a Solid • Particles in a solid are PACKED CLOSELY together and they are in a FIXED POSITION. Particles vibrate in place
- 7. Liquids • Liquids – has definite VOLUME but no defined SHAPE 100 ml
- 8. Gases • Gases - do NOT have definite SHAPE or VOLUME. Bromine gas fills up the entire volume of the container
- 9. Particle view of a Gas • Particles can MOVE FREELY and will either fill up or squeeze into available space.
- 10. Questions • 1) Which Statement is True? – A) Liquids have a definite shape and volume – B) States of matter are defined by the substances they are made up of – C) Gases have a definite shape and volume – D) Solids have a definite shape and volume
- 11. Task • Draw a diagram of – A) Gas particles – B) Liquid particles – C) Solid particles
- 12. Changes in States of Matter • Thermal Energy – heat energy. • More thermal energy = More particle movement
- 13. Changing States Increase Thermal Energy (Heat up) Solid Liquid Gas Decrease Thermal Energy (Cool off)
- 14. Melting point • Melting - change from solid to liquid • Melting point - SPECIFIC temperature when melting occurs. • Each pure substance has a SPECIFIC melting point. – Examples: – M.P. of Water = 0°C (32°F) – M.P. of Nitrogen = -209.9 °C (-345.81998 °F) – M.P. of Silver = 961.93 °C (1763.474 °F) – M.P. of Carbon = 3500.0 °C (6332.0 °F)
- 15. Melting Point • Particles of a solid vibrate so fast that they break free from their fixed positions. Increasing Thermal Energy Solid Liquid Melting point
- 16. Vaporization • Vaporization – change from liquid to gas • Vaporization happens when particles in a liquid gain enough energy to form a gas. Increasing Thermal Energy Liquid Gas Boiling point
- 17. Two Kinds of Vaporization • Evaporation – vaporization that takes place only on the surface of the liquid • Boiling – when a liquid changes to a gas BELOW its surface as well as above.
- 18. Boiling Point • Boiling Point – temperature at which a liquid boils • Each pure substance has a SPECIFIC boiling point. – Examples: – B.P. of Water = 100°C (212°F) – B.P. of Nitrogen = -195.79 °C (-320.42 °F) – B.P. of Silver = 2162 °C (3924 °F) – B.P. of Carbon = 4027 °C (7281 °F)
- 20. • The Kinetic Molecular Theory explains the forces between molecules and the energy that they possess. This theory has 3 main points : – Matter is composed of small particles (atoms or molecules). • • • Particles are moving all the time.(higher Temp. higher of average energy – The molecules are in constant motion. This motion is different for the 3 states of matter. –
- 21. Boiling Point and Melting Point Melting point Boiling point
- 22. Solubility • Maximum amount of a substance that can be dissolved in a liquid (at a specific temperature). Salt (NaCl) Water (H20) at 20°C
- 23. Solubility • Solute – substance being dissolved • Solvent – liquid substance that solute is dissolved into Salt (NaCl) Water (H20) at 20°C
- 24. Solubility • Solute – ?????? • Solvent – ????? Salt (NaCl) Water (H20) at 20°C Salt Water
- 25. Solubility can change • Increased Temp = Increased Solubility • Different substances have different solubility curves Solubility of Unknown Substance at different temperatures 3 unknown 2.5 2 1.5 of 1 mg 0.5 0 temperature (degrees Celcius) 1 3.8 6.6 9.4 12.2 15 17.8 20.6 23.4 26.2 substance/ml of H20
Editor's Notes
- This fixed, closely packed arrangement causes a solid to have a definite shape and volume