1. Warm Up – 9/18
Conversion Practice 2.5 Km = ________________ cm 4.67 mm = ___________________ m 5.89 L = _________________ ml 15m = ____________________mm 26ml = ____________________ L

2. Warm-Up 9/25 Compare covalent and ionic bonding What are isotopes?
Define: Compound
Provide one example of a chemical formula.

3. Warm Up 10/1
What is Cohesion and Adhesion? Provide one example of each.

4. The Nature of Matter & Biomolecules
Chapter 2
The Nature of Matter & Biomolecules

5. Living things consist of atoms of different elements.
Matter - anything that occupies space and has mass
An element is one type of atom, cannot be broken down into other substances. H O
Essential VS Trace Elements???
Hydrogen atom (H)
Essential Elements:
C, H, O, N = 96%
P, Ca, K, S = ~4%
Oxygen atom (O)
Trace Elements: > 0.01 %
ex: iodine, iron, copper, etc.

6. Atoms Three subatomic particles make up atoms. Protons Neutrons
Electrons
100 million atoms side by side would make a row—about the width of your little finger!

7. Protons and Neutrons Protons and neutrons have about the same mass.
Protons = positively charged particles (+)
Neutrons = neutral particles (No net charge)
Nucleus is the center of the atom
Made of both protons and neutrons
Protons and neutrons are held in the
nucleus by the strong force.

8. Electrons Negatively charged particle (–) Extremely small
1/1840 the mass of a proton.
Attracted to the positively charged nucleus and are inconstant motion around the nucleus.

9. Electrons Electrons are in energy levels outside nucleus.
The first energy level can hold two electrons
The second energy level can hold up to eight.
2n2 = # of electrons an energy level can hold
Oxygen atom (O)
Nucleus: 8 protons (+) 8 neutrons
outermost energy level: 6 electrons (-)
inner energy level: 2 electrons (-)

10. Atoms In general atoms have equal numbers of electrons and protons.
The positive and negative charges balance out.
Atoms are electrically neutral.
The carbon atom shown has 6 protons and 6 electrons.
Atomic Basics Video

11. Elements
Element - a pure substance that consists entirely of one type of atom.
Elements represented are one- or two-letter symbols.
Example:
C for carbon
H for hydrogen
Na for sodium
Hg for mercury
Over 100 Elements known!!

12. Atomic Basics
Atomic number - The number of protons in the atoms nucleus
Carbon’s atomic number is 6
What does this mean?
Each atom of carbon has _____ # of:
Protons =
Electrons =
Protons ___ + Neutrons ___ = _____ Atomic Mass
Atomic Mass – Total number of protons and neutrons in and atoms nucleus. 6 6 12

13. Isotope
Isotope - Atoms of the same element that differ in the number of neutrons
Atoms of carbon have 6 neutrons. Some can have 7 or 8. These are isotopes of carbon
Isotopes are identified by their mass number.
carbon-12, carbon-13, and carbon-14.

14. Radioactive Isotopes
Radioactive means - that their nuclei are unstable and break down at a constant rate over time.
Practical Uses for Radioactive Isotopes
Geologists can determine the ages of rocks and fossils by analyzing the isotopes found in them.
Radiation from certain isotopes can be used to detect and treat cancer
To kill bacteria that cause food to spoil.
Labels or “tracers” to follow the movements of substances within organisms.

15. Chemical Compounds Food for Thought!
The physical and chemical properties of a compound are usually very different from those of the elements from which it is formed.
What elements are pictured below?

16. Chemical Compounds Example:
Sodium is a silver-colored metal that is soft enough to cut with a knife. It reacts explosively with cold water.
Chlorine is a very reactive, poisonous, greenish gas that was used in battles during World War I.
However, the compound sodium chloride--table salt--is a white solid that dissolves easily in water, is not poisonous, and is essential for the survival of most living things.

17. Compounds
Compound - a substance formed by the chemical combination of two or more elements in fixed proportions.

18. Chemical Bonds Two main types of chemical bonds Ionic bond
Covalent bond

19. Ionic Bond
Ionic bond - formed when one or more electrons are transferred from one atom to another.
Atom that loses electrons = positively charged.
The atom that gains electrons = negatively charged.
Ions = positively and negatively charged atoms

20. Ionic Bond Example

21. Ionic Bond Example

22. Ionic Bond Example

23. Ionic Bond Example
These oppositely charged ions have a strong attraction for each other, forming an ionic bond.
Dogs Teach Chemistry - Ionic Bond Video

24. Covalent Bonds
Covalent Bond – Formed when pairs electrons are shared by atoms
The shared electrons travel around both nuclei!
Single Bond = share two electrons
Double Bond = share four electrons.
Triple Bond = share six electrons,
2 Oxygen Atoms = O2

25. Molecules
Molecules - when 2 or more atoms are held together by covalent bonds.
Chemical formula - Shorthand writing of the elements and number of atoms in a compound.
Water contains two atoms of hydrogen for each atom of oxygen
Chemical formula - H2O.
The formula for table salt - NaCl
Sodium (Na) –
Chlorine (Cl) –
Combine in a 1:1 ratio

26. Molecules
Structural formula: shows types of atoms in a molecule and how they are bonded together.

27. PRACTICE!!!
Determine if each is the chemical or structural formula of the molecule.
KMnO4
MgSO4
Acetone

28. Chemical Reactions
Chemical reaction: The breaking of old bonds and forming of new chemical bonds.
Reactants: starting materials for a reaction
Products: ending materials from a reaction =

29. Objectives 2.2 2.2 Properties of Water
Describe the structure of a water molecule
List and describe water’s unique properties
Distinguish between an acid and a base
Explain how Earth’s conditions are fit for life

30. The Water Molecule
Key Topic!
How does the structure of water contribute to its unique properties?

31. Polarity
The oxygen atom has a greater attraction on the shared electrons.
As a result:
The oxygen end of the molecule has a slight negative charge
The hydrogen end of the molecule has a slight positive charge.
This is called a polar molecule

32. Hydrogen Bonding
Hydrogen bond – attraction between a hydrogen atom on one water molecule and the oxygen atom on another.

33. Hydrogen Bonding Water can form multiple hydrogen bonds
Not as strong as covalent or ionic bonds
Can form in other compounds besides water.
DNA

34. Properties of Water
Hydrogen bonds are responsible for three important properties of water.
high specific heat (1 calorie/gram °C = joule/gram °C)
Cohesion: tendency of like molecules to stick together
Adhesion: type of attraction that occurs between unlike molecules

35. Cohesion
Cohesion - an attraction between molecules of the same substance.
a single water molecule can form up to four hydrogen bonds simultaneously
Water is extremely cohesive.

36. Cohesion
Cohesion causes water molecules to be drawn together, which is why drops of water form beads on a smooth surface.
Cohesion also produces surface tension, explaining why some insects and spiders can walk on a pond’s surface.

37. Adhesion
Adhesion - an attraction between molecules of different substances.
The surface of water is attracted to the glass of the graduated cylinder
Causing the meniscus

38. Cohesion & Adhesion
Adhesion: attraction that occurs between unlike molecules
Cohesion: tendency of like molecules to stick together

39. Heat Capacity
Heat capacity - The amount of heat energy required to increase its temperature.
Relatively high compared to other compounds
Examples
Large bodies of water, such as oceans and lakes, can absorb .
This protects organisms living within from dramatic changes in temperature.
At the cellular level, water absorbs the heat produced by cell processes, regulating the temperature of the cell.
Water Properties Video

40. Dissolving compounds in water.
Solution - when one substance dissolves in another.
Solvents - dissolve other substances. (H2O)
Solutes - dissolve in a solvent. (NaCl)
Aqueous Solution – any solution where water is the solvent.
solution

41. Solutions “Like dissolves like.”
Polar solvents dissolve polar solutes.
Nonpolar solvents dissolve nonpolar solutes.
Polar substances and nonpolar substances generally remain separate.
They don’t mix!!
Explain why some salad dressings needs to be shaken before you use them.

42. Acids, Bases, and pH
Water molecules sometimes split apart to form hydrogen ions and hydroxide ions.

43. The pH Scale
pH scale - indicates the concentration of H+ ions in solution.
The pH scale ranges from 0 to 14.
< 7 = Acidic
7 = Neutral
> 7 = Basic

44. Acids Acid - any compound that forms H+ ions in solution.
pH values below 7
High levels of H+ ions
Strong acids tend to have pH values that range from 1 to 3. Hydrochloric acid (HCl) is a strong acid produced by the stomach to help digest food.

45. Bases
Base – any compound that produces hydroxide (OH–) ions in solution.
pH values above 7
Basic, or alkaline, solutions contain low concentrations of H+ ions.

46. The pH Scale