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Hydrogen bonds form between neighboring water molecules

2 x (Hydrogen -1O)

Oxygen - 2H

Each water molecule can hydrogen-bond to up to 4 partners.

Raised by Polarity

H atoms are attached to O atoms by polar covalent bonds

Because of the polar bonds and wide V shape, water is a polar molecule with→ unequal distribution of charges

O end → slightly negative , H end → slightly positive

Hydrogen is attracted to a nearby atom like O (or N) → H bonds

weaker bonds than covalent

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Adhesion: Water sticks to all sorts of things, making them wet—cotton jeans, soil, your hair. When water sticks to some other substance, like cotton, it is called adhesion.
Cohesion: Water also sticks to itself, as evidenced by a drop of water dripping from a faucet or falling from a cloud. Cohesion is the tendency of water molecules to stick to each other.
hydrogen bonds
hydrophilic: Substances that dissolve in water or are attracted by water are called hydrophilic. This property is also the result of water “sticking” to hydrophilic substances.
hydrophobic: Substances that do not dissolve in water or repel water are called hydrophobic. Both hydrophilic and hydrophobic substances can be found in living systems.
polar covalent bond
O's - charge: An oxygen atom has a greater affinity or attraction for electrons than a hydrogen atom does. Therefore, when a hydrogen atom and an oxygen atom share a pair of electrons in a chemical bond, the electrons spend more time around the oxygen nucleus than they do around the hydrogen nucleus. The unequal sharing of electrons creates two separate areas of electrical charge. Around the oxygen atom the molecule is partially negatively charged with more electrons, more of the time. Around the hydrogen atoms the molecule is partially positively charged because the electrons spend less time there.

EXAMPLES:  place a pan of water on the stove and turn the burner to high. Wait 30 seconds. The pan reaches burning temperatures much faster than the water does. This demonstrates that water resists changes in temperature more than steel does.

in Seattle or Boston, which are both along seacoasts, the temperatures rarely get above 100 degrees Fahrenheit or below zero. On the other hand, cities in the U.S. heartland, such as Minneapolis or Omaha, experience these temperatures on a yearly basis. Without the huge oceans, Earth’s temperatures would not be compatible with life as we know it.

because ice floats, a thin layer of ice insulates the rest of a lake, allowing aquatic life to survive the winter. Think about that the next time you are clinking ice cubes in your soft drink.

Your cells are essentially small packets of water that contain a complex solution of molecules dissolved within the water.
Two substances you are familiar with that do not dissolve in water are waxes and oils. Water beads up on waxy surfaces and the oil in salad dressing rises above the watery vinegar.

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Using Energy (Metabolism/ Energy processing) Examples

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Using Energy (Metabolism/ Energy processing) Examples

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Water's Life supporting properties are related to:
-structure
-Interaction of its molecules
-Polarity
-H bonding (Raised by Polarity)

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2 or more atoms held together by covalent bonds

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Measure of an atom's attraction for shared e-

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E- are shared equally because the two atoms have the same electronegativity.

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-> E- are not shared equally because the two atoms don't have the same electronegativity.
-> e- are drawn more closely to the more electronegative element (O).
-> An atom carries a partially - charge other a partially + charge.

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-> e- are given / taken (transfer) result in attraction

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-> e- are shared.
-> Strong bonds.
-> Found in molecules
-> bonding capacity depends on valence

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Electrons can be located in different shells. Atoms gain, loose, or share e- to fill their outer e- shell.

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Acid-Base Balance

Body Temperature

Glucose Concentration

Calcium Levels

Fluid Volume

maintenance of healthy blood pressure

lymphatic system fights infection and maintains health

maintaining balance of water

Calcium levels in the blood

nervous system balances breathing patterns (involuntary)

body eliminates indigestible & dangerous substances through urinary & digestive systems. An individual urinates and defecates toxins from the blood.

https://examples.yourdictionary.com/homeostasis-examples.html

https://www.brighthub.com/science/medical/articles/112024/

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Iron to cereals, iodine is in the salt that we eat, fluorine to tap water...

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boron
chromium
cobalt
copper
fluorine
iodine
iron

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salt -> NaCl
Water -> H20
Carbon dioxide -> C02
glucose -> C6H1206

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hydrogen
copper
carbon
oxygen
iron
aluminum
magnesium

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MATTER: Anything that occupies space and takes up mass.
COMPOUND:  A substance consisting of two or more different elements in a fixed ratio.
ATOM: The smallest unit of matter that still retains the properties of an element.
NUCLEUS: An atom's central core, containing protons and neutrons.
PROTON: A subatomic particle with a single positive electrical charge (+).
NEUTRON: A subatomic particle with no charge.
ELECTRON: A subatomic particle with a single negative charge (-).
TRACE ELEMENTS: Elements present in the body in small quantities (<0.01%).

ATOMIC NUMBER: The number of protons in each atom of a particular element.
ATOMIC MASS: The total mass of an atom.
MASS NUMBER: The sum of the number of protons and neutrons in an atom's nucleus
CHEMICAL BOND: A type of strong chemical bond in which two atoms share one or more pairs of valence electrons.
IONIC BOND: A chemical bond resulting from the attraction between oppositely charged ions.
COVALENT BOND: An attraction between two atoms resulting from a sharing of outer-shell electrons or the presence of opposite charges on atoms.
ELECTRON SHELL: A level of electrons at a characteristic average distance from the nucleus of an atom.
ISOTOPE: One of several forms of an element, each with the same number of protons but a different number of neutrons.
RADIOACTIVE ISOTOPE: An isotope whose nucleus decays spontaneously, giving off particles and energy.

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Sweating is

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Organization (Order), living things are made up of cells Examples

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Organization (Order), living things are made up of cells Examples

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- Growth and Development
- Reproduction
- Adaptation (Evolutionary Adaptation)
- Response to Stimuli
- Using Energy (Metabolism/ Energy processing)
- Maintaining Homeostasis (Regulation)
- Organization (Order)